Chemistry Of Matter Chemistry; Study Of Matter Chemistry – Flashcards
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What is an Element?
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It is a pure substance that cannot be broken down into two or more simpler substances by chemical processes.
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Metal (appearance)
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Shiny (Lustrous)
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Metal (Physical state at R.T.P)
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Mostly solids (except mercury)
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Metals (melting and boiling points)
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High (except for sodium, potassium and mercury)
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Metals (Heat and electrical conductivity)
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Good
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Metalloids (Appearance)
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Shiny (Lustrous)
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Metalloids (Physical state at R.T.P.)
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Solids
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Metalloids (Melting and boiling points)
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High
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Metalloids (Heat and electrical conductivity)
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Moderate
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Non-metal (appearance)
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dull (non-lustrous)
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Non-metal (Physical state at R.T.P)
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Gases, volatile liquids or solids
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Non-metal (Melting and Boiling points)
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Low (except for carbon and silicon)
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Non-metal (Heat and electrical conductivity)
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Poor (except carbon in the form of graphite and diamond)
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Metals (ductility and malleability)
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Ductile, Malleable and Sonorous
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Metalloids (ductility and malleability)
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Brittle
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Metalloids (ductility and malleability)
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brittle
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What is Ductile?
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Can be drawn into wires
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What is Malleable?
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Can be hammered into different shapes without breaking
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What is Sonorous?
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Makes a ringing sound when struck
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What is Brittle?
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Easily broken when hammered
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An element is made up of?
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An element is made up of tiny particles called atoms
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What are atoms?
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Atoms are the smallest particles of an element that have the chemical properties of that element
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1 property about the atom
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The atom of an element are different from that of another element
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What is a molecule?
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It is a group of two or more atoms that are chemically combined
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What are diatomic molecules?
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Diatomic molecules are those that are formed by the combination of two atoms
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Some examples of diatomic molecule
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Hydrogen, oxygen, nitrogen
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What are polyatomic molecules?
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Polyatomic molecules consists of three or more atoms that are chemically combined together
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What is a compound?
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A compound is a pure substance that contains two or more elements that are chemically combined in a fixed ratio
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Characteristics of compound (Number 1)
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A compound has different properties from the elements that form it
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Characteristics of compound (Number 2)
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A chemical reaction is necessary to separate the elements in a compound
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Characteristics of compound (Number 3)
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Every compound has fixed compositions of the different elements it contains
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Characteristics of compound (Number 4)
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A chemical reaction takes place in the formation of compounds
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What will a chemical change / chemical reaction produce?
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It would produce one or more new compounds which have different properties from the initial components
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Chemical change is / causes?
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It is irreversible, new substances are formed, light and / or heat energy is given out and the properties of products are different from starting reactants
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What is physical change?
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A change in which no new compounds is formed
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What are mixtures?
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Mixtures are made up of two or more substances that are not chemically combined
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What is a alloy?
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It is a mixture of metals with other elements (usually metals but sometimes non-metal such as carbon)
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Characteristics of Alloys (Number 1)
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Stronger than pure metals
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Characteristics of Alloys (Number 2)
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Similar chemical properties to elements they contain
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Characteristics of Alloys (Number 3)
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Different physical properties
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Properties of Mixtures (Number 1)
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A mixture can be separated easily by physical methods (without involving chemical reaction)
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Properties of Mixtures (Number 2)
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The components in mixtures are not mixed in any fixed proportion
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Difference between Mixture and Compound (energy change)
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No chemical reaction takes place when a mixture is formed, usually there is little or no energy change, while a chemical reaction takes place when a compound is formed, usually there is an energy change
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Difference between Mixture and Compound (Composition)
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The components of a mixture can be mixed in any proportion while the elements in a compound are always combined in a fixed proportion
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Difference between Mixture and Compound (Separation)
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The components of a mixture can be separated by physical processes such as magnetic separation, filtration or distillation while a compound can only be broken down into its elements or into simpler compounds by chemical processes
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Difference between Mixture and Compound (Properties)
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The chemical properties of a mixture are the same as those of its components while the physical and chemical properties of a compound are different from those of its constituent elements.
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anything that has mass and volume
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matter
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the measure of the quantity of matter
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mass
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the measure of the space occupied by matter
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volume
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study of matter
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chemistry
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mass can not be created or destroyed in a physical or chemical change
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Law of Conservation of Matter
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mass of products
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mass of reactants =
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matter that has uniform composition and definite composition
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substance
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properties do not vary throughout sample
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uniform composition
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always the same from sample to sample
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definite composition
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2 types of substances
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elements and compounds
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simplest form of matter, composed of a single kind of atom, can't break into simpler substances by chemical means
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element
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represented by chemical symbols
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element
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substance composed of elements that are chemically combined, can be broken down into simpler substances by chemical means
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compound
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represented by a chemical formula
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compound
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2 types of compounds
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Ionic and Covalent
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composed of positive and negatively charged particles called ions
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ionic compound
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composed of particles called molecules
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covalent compound
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a physical combination of two or more substances which maintain their properties
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mixture
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can be separated by physical means by filtration or distillation
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mixture
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two types of mixtures
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heterogenous and homogenous
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not uniform composition, portions not alike, separated by filtration
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heterogeneous mixture
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uniform composition, portions alike, separated by distillation
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homogenous mixture
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3 states of matter
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solids, liquids, gases
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With a change in ____, a substance in one state may change to another state.
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temperature
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changing from one state to another
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physical change
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all matter is composed of tiny particles that are in constant motion
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Kinetic Theory of Matter
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the higher the temperature the greater the motion/solids,liquids, and gases differ in motion of particles and how strongly they are attracted to one another
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Kinetic Theory of Matter
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definite volume, definite shape/particles strongly attracted ; arranged in organized patterns
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solids
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vibrational motion only/ incompressible
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solids
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Solids will turn to liquids at their ________.
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melting point temperature
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definite volume, indefinite shape/ particles slide over each other
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liquids
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vibrational and rotational motion only/almost incompressible
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liquids
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Liquids will turn to gases at their ______.
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boiling point temperature
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indefinite volume, indefinite shape/ particles not attracted - move in straight line till they collide
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gases
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vibrational, rotational, and translational motion/compressible
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gases
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help chemists identify substances
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physical and chemical properties
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observed or measured without changing the composition of a substance/no reaction
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physical properties
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density, color, boiling point, solubility, volume, mass, temperature, odor
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physical properties examples
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a change which alters a substance but not its composition (generally appearance)
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physical change
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describes the reaction of substances/ new substances formed
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chemical properties
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one or more substances change into new substances
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chemical change
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technique that separates components in a mixture by particle size
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filtration
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separates using boiling point
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distillation
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a property that describes how a substance reacts with another substance
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chemical property
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used to observe and describe matter
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physical property
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most reactive group of metals
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alkali metals (group 1A)
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fairly reactive group of metals
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alkaline earths
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most reactive group of non metals
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halogens (group V11A)
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unrective group of non-metals
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noble inert gases
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Workplace, Hazardous, Material, Information,System
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WHMIS
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Material, Safety, Data, Sheets
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MSDS
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the elements along the staircase. elements with properties of both metal and non metals
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metalloids
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compounds are always combined together in fixed proportions ex; H20
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Law Of Definite Proportions
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pure substances that are made up of two or more elements combined together to form a molecule
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compounds
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grouping elements with similar physical and chemical properties ex; alkali metals, alkaline earths, halogens, nobel (inert) gases
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chemical family
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(physical property) described using words ex; she has BLUE eyes
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qualitative
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a pure substance made up of one type of particle, or atom
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element
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the study of matter and how we can make changes to matter
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chemistry
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anything that takes up space or contains mass
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matter
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a substance changes in form but not in composition ex; ice to water the change can be easily reversed; freeze water to create ice
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physical change
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when one or more new substances are created; a change that is impossible to reverse ex; cooking
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chemical change
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the substances that go into a chemical reaction
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reactants
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the substances produced by a chemical reaction
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products
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1. all matter is made up of very tiny particles 2. all particles are moving 3. all particles are different from each other 4. all particles are attracted to each other 5. the speed of how fast the particles are moving is determined by the temperature
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particle model of matter
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combination of two or more pure substances
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mixture
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a material containing one particle ex; water
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pure substance
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the particles in the mixture remain intake and are not uniformly scattered throughout ex; granola bar (heterogeneous)
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mechanical mixtures
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the particles in this mixture are uniformly scattered ex; apple juice is (homogeneous)
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solution
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substance and mixture which are in a single phase ( cannot see all the particles) ex; apple juice ( solution)
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homogeneous
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a substance dissolved in another substance ex; salt water the solute is the salt
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solute
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physical property that can be described using numbers ex; the boiling temperature ex; he has size 11 feet
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quantitative
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an element incapable of forming simple positive ions in a solution ex; gases
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non metal
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any of the electropositive elements that usually have a shiny surface are good conductors of heat and electricity
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metals
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decomposing a chemical compound by passing electricity through it
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electrolysis
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the liquid substance in a solution ex; salt water the water is the solvent in this mixture
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solvent
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a mixture that contains two or more substances ( you can actually see two or more substances)ex; granola bar
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heterogeneous
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in a chemical change the total mass of the new substance is always the same as the total mass of the original substance ( Lavoisier)
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Law Of Conservation of Mass
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compound that gives off H+ ions in solution
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acid
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describes a solution with a high concentration of H+ ions
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acidic
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ions with a negative charge
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anion
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the electrode where electrons are lost (oxidized) in redox reactions
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anode
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common units for measuring pressure
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atmospheres
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the smallest object that retains properties of an element. Composed of electrons and a nucleus (containing protons and neutrons)
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atom
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number of protons in an element
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atomic number
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number representing the number of molecules in (1) mole: 6.022 * 10 to the 23 power
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Avogadro's number
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substance which gives off hydroxide ions (OH-) in solution
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base
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having the characteristics of a base
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basic
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He made significant contributions to the atom. He understood the line spectra--the reason why only certain wavelengths are emitted when atoms jump down levels
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Bohr's atom
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solutions that resist change in their pH, even when small amounts of acid or base are added
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buffer solutions
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substances that speed up a chemical process without actually changing the products of reactions
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catalyst
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electrode where electrons have gained (reduction) in redox reactions
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cathode
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ion with positive charge
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cations
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in a Lewis structure, usually the atom that is the least electronegative
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central atom
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describes an object's ability to repel or attract other objects. Protons have a positive ...while electrons have a negative... Like ...repel each other, while opposites attract.
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charge
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processes or events that have altered the fundamental structure of something
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chemical changes
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an expression of a fundamental change in the chemical substance
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chemical equation
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properties of a solution that depend only on the number of particles dissolved in it, not the properties of the particles themselves. The main ones are boiling point elevation and freezing point depression.
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colligative properties
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when substances combine with oxygen and release energy
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combustion
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two or more atoms joined together chemically, with covalent or ionic bonds
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compound
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the amount of a substance in a specified space
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concentration
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a substance which can lose H+ ion to form a base
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conjugate acid
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a substance which can gain H+ ion to form an acid
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conjugate base
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when two atoms share at least one pair of electrons
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covalent bonds
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change of an element into a different element, usually with some other particle(s) of energy emitted
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decay
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mass per unit volume of a substance
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density
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intermolecular forces that exist between polar molecules. Active only when the molecules are close together. The strengths of intermolecular attractions increase when polarity increases
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dipole-dipole forces
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dispersion is an intermolecular attraction force that exists between all molecules. These forces are the result of the movement of electrons which cause slight polar moments. Generally very weak, when their molecular mass increases, so does their strength
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dispersion forces (London dispersion forces)
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breaking down of a compound into its components to form ions from an ionic substance
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dissociation
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when an atom is bonded to another atom by two sets of electron pairs
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double bond
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movement of gas molecules through a small opening
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effusion
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gives an electric current with a steady voltage as a result of an electron transfer reaction
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electrochemical cell
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device that moves electrons into or out of a solution by conduction
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electrodes
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changing the chemical structure of a compound using electrical energy
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electrolysis
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complete range of wavelengths which light can have. These include infrared, ultraviolet and all other types of radiation as well as visible light
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electromagnetic spectrum
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one of the parts of an atom having a negative charge. Indivisible particle with a charge of -1
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electrong
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measure of a substance's ability to attract electrons
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electronegativity
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forces between charged objects
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electrostatic forces
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substance consisting of only one type of atom
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element
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formula showing the simplest ratio of elements in a compound
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empirical formula
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process that absorbs heat from its surroundings as the reaction proceeds
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endothermic
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ability to do work
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energy
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change in heat at constant pressure
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enthalpy
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measure of the disorder of a system
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entropy
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when the reactants and products are in a constant ratio. The forward reaction and the reverse reactions occur at the same rate when a system is in this state
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equilibrium
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value that expresses how far the reaction proceeds before reaching equilibrium. A small number means that equilibrium is towards the reactants side while a large number means that the equilibrium is towards the product side
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equilibrium constant
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the expression giving the ratio between the products and reactants. It is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divided by the concentration of the product of reactants to the power of their coefficients
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equilibrium expression
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occurs when the moles of acid equal the moles of base in a solution
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equivalence point
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process that gives off heat to the environment
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exothermic
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number of events in a given unit of time. When describing a moving wave, means the number of peaks which would pass a stationary point in a given amount of time
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frequency
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instrument that measures radiation output
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Geiger counter
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the energy of a system that is available to do work at a constant temperature and pressure
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Gibb's free energy
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the rate of diffusion of a gas is inversely proportional to the square root of its molar mass
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Graham's law
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the amount of time it takes for half an initial amount to disintegrate
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half life
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the principle states that it is not possible to know a particle's location and momentum precisely at any time
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Heisenberg uncertainty principle
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strong type of intermolecular dipole-dipole attraction. Occurs between hydrogen and F, O or N
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hydrogen bonding
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the reactions of cations with water to produce a weak base or of anions to produce a weak acid
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hydrolysis
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forces between molecules
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intermolecular forces
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forces within molecules. Forces caused by the attraction and repulsion of charged particles
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intramolecular forces
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removing or adding electrons to an atom creates an ... (a charged object very similar to an attom)
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ion
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when two oppositely charged atoms share at least one pair of electrons but the electrons spend more time near one of the atoms than the other
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ionic bond
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energy required to remove an electron from a specific atom
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ionization energy
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elements with the same number of protons but have different numbers of neutrons, and thus different masses
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isotopes
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The SI unit of temperature. It is temperature in degrees Celsius plus 273.15
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Kelvin
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energy an object has because of its mass and velocity. Objects that are not moving do not have this.
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kinetic energy
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states that a system at equilibrium will oppose any change in the equilibrium conditions
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Le Chatlier's Principle
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a way of representing molecular structures based on valence electrons
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Lewis structures
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the reactant that will be exhausted first
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limiting reagent
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the number of protons and neutrons in an atom
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mass number
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composed of two or more substances, but each keeps its original properties
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mixture
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the number of moles of solute (the material dissolved) per kilogram of solvent (what the solute is dissolved in)
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molality
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a term expressing molarity, the number of moles of solute per liters of solution
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molar
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the number of moles of solute (the material dissolved) per liter of solution. used to express the concentration of a solution
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molarity
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a collection of 6.022 * 10 to the 23 power number of objects. Usually used to mean molecules
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mole
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shows the number of atoms of each element present in a molecule
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molecular formula
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shape of a molecule, based on the relative position of the atoms
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molecular geometry (VSEPR)
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the combined mass (as given on the periodic table) of all the elements in a compound
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molecular mass
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two or more atoms chemically combined
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molecule
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the number of moles of a particular substance expressed as a fraction of the total number of moles
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mole fraction
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an object that does not have a positive or negative charge
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neutral
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a particle found in the nucleus of an atom. It is almost identical in mass to a proton, but carries no electrical charge
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neutron
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abbreviation for nanometers. A nanometer is equal to 10 to the -9 power meters
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nm
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the central part of an atom that contains the protons and neutrons. Plural=nuclei
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nucleus
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In Lewis structures, the goal is to make almost all atoms have this structure. This means they will have access to (8) electrons regularly, even if they do have to share some of them
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octet
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an energy state in the atomic model which describes where an element will likely be
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orbitals
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a number assigned to each atom to help keep track of the electrons during a redox-reaction
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oxidation number
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a reactions involving the transfer of electrons
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oxidation-reduction-reaction
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an element that undergoes nuclear decay
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parent isotopes
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the pressure exerted by a certain gas in a mixture
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partial pressure
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small portion of matter
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particle
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expresses the mass ratio between different elements in a compound
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percent composition
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grouping of the known elements by their number of protons. There are many other trends such as size of elements and electronegativity that are easily expressed in terms of the periodic table
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periodic table
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measures the acidity of a solution. It is the negative log of the concentration of the hydrogen ions in a substance
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pH
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massless packet of energy, which behaves like both a wave and a particle
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photon
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a property that can be measured without changing the chemical composition of a substance
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physical property
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What is h?
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Planck
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He contributed to the understanding of the
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Planck
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Measures the basicity of a solution. It is the negative log of the concentration of the hydroxide ions
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pOH
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Molecule with a partial charge
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polar molecules
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The energy an object has because of its composition or position
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potential energy
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Force per unit area
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pressure
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The number related to the amount of energy an electron has and therefore describing which shell the electron is in
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principal quantum number (n)
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The compounds that are formed when a reaction goes to completion
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products
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An equality between two ratios
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proportion
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Particle found in a nucleus with a positive charge. Number of these gives the atomic number
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proton
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Something that comes in discrete units
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quantum
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Set of numbers used to completely describe an electron
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quantum numbers
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Energy which is transmitted away from its source, for example, energy that is emitted when electrons transition down one level to another
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radiant energy
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Energy in the form of photons
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radiation
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Substance containing an element which decays
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radioactive
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The relative size of two quantities expressed as the quotient of one divided by the other; a:b or a/b
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ratio
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Substances initially present in a chemical reaction
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reactants
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A reaction in which a substance gains at least one electron
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reduction reaction
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Ionic compounds that can be formed by replacing one or more of the hydrogen ions of an acid with another positive ion
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salts
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Where the electrons generally are; they are composed of four types of sub...; s, p, d and f
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shells (orbitals)
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When an electron pair is shared by two atoms
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single bond
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Standards for Systeme International d'Unites, an international system which establishes a uniform set of measurement units
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SI Unit
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The substance (solid, liquid or gas) dissolved in a solution, for example, the salt in saltwater
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solute
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Mixture of a solid and a liquid where the solid never settles out, for example, saltwater
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solution
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Liquid in which something is dissolved, for example the water in saltwater
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solvent
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The amount of heat it takes for a substance to be raised by one degree Celsius
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specific heat
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A reaction that will proceed without any outside energy
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spontaneous reaction
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Solid, liquid, gas and plasma. Plasma is a "soup" of disassociated nuclei and electrons, normally found only in stellar objects
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states of matter
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The study of the relationships between amounts of products and reactants
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stoichiometry
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Standard Temperature and Pressure. 0 degrees Celsius and 1 atm
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STP
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One part of a level, each of which can hold different numbers of electrons
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subshell (suborbital)
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The study of temperature, pressure, volume and energy flow in chemical reactions
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thermodynamics
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The process used to take a solution of unknown concentration with a solution of a known concentration for the purpose of finding out more about the unknown solution
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titration
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The electrons in the outermost shell of an atom
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valence electrons
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An equation for non-ideal gases that accounts for intermolecular attraction and the volumes occupied by gas molecules
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van der Waals equations
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Speed of an object; the change in position over time
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velocity
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Measures the size of an object using length measurements in three dimensions
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volume
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A signal which propagates through space
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wave
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On a periodic curve, the length between two consecutive troughs (low points) or peaks (high points)
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wavelength
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Substances capable of donating hydrogen but do not completely ionize in solution
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weak acid
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Substances capable of accepting hydrogen but do not completely ionize in solution
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weak bases
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Expression of the movement of an object against some force
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