Intro into Chemistry – Flashcards

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Natural Laws
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concise statements often in mathematical form about natural phenomenon
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hypothesis
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tentative explanation of a natural law
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Theory
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model or way of looking at nature that can be used to explain natural laws and make future predictions about natural phenomina
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Scientific Method
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combination of observation, experimentation, and formulation of laws, hypotheses and theories
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Chemistry
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Science that deals with the composition and properties of matter
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Matter
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anything that occupies space and displays the properties of mass and energy(inertia)
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Compostition
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refers the the parts of compounds of a sample of matter and their relative proportions
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Properties
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re those qualities or attributes that we an use to distinguish one sample of matter from another
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Physical Property
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is one that a sample of matter displays without chaninging its composition i.e. color staying the same and so forth
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Physical Change
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when the physical properties of a subject change but its composition stays the same
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Chemical Change(reaction)
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when one or more kinds of matter are converted to new kinds of matter with different compositions
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Chemical Property
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the ability or inability of a sample of matter to undergo a change in composition under stated conditions
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Atoms
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the very tiny units that make up matter
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Elements
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114 substances of atoms that make up these pieces that make matter
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Compounds
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substances comprised of atoms of two or more elements joined together
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Molecule
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the smallest entity having the same proportions of the constituent atoms as does the compound itself
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Substance
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is a element or compound that has constant properties throughout a a given sample and from one sample to another
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Homogeneous mixture
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a solution said to be uniform throughout in both composition and properties
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Heterogeneous mixtures
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(i.e. sand and water) components of a substance that separate into distinct regions
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Solid
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where atoms and molecules are in close contact, in sometimes highly organized sections called crystals
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Liquid
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where the atoms or molecules are separated in somewhat greater distances than that of a solid
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Gas
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distances of molecules and atoms are very much spread apart. Gas always expands to full container
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SI Units
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Ssteme Internationale d'Unites, which is the modern version of the metric system used for scientific measuring
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Define Units and symbol of Length
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meter m
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Define Units and symbol of Mass
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kilogram kg
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Define Units and symbol of Time
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second s
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Define Units and symbol of Temperature
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kelvin K
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Define Units and symbol of Amount of Substance
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mole mol
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Define Units and symbol of Electric Current
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ampere A
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Define Units and symbol of luminous intensity
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candela cd
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10^1
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deca(d)
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10^2
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Hecto(h)
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10^3
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Kilo(k)
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10^6
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Mega(M)
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10^9
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giga(G)
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10^12
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Tera(T)
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10^-1
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Deci(d)
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10^-2
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centi(c)
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10^-3
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milli(m)
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10^6
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micro
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10^9
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nano(n)
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Mass
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describes the quantity of matter in an object. In SI, mass= 1gram
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Celsius
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melting point of ice is 0 degrees while the oiling point is 100
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Fahreneit
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melting point of ice is 32 degress and the boiling point is 212
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Kelvin
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assigns a value of zero to the lowest possible temperature. No negative Kelvin numbers
-273.15C =0K
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Density
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ration of mass to volume, aka mass(m)/volume(v)
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Extensive property
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where mass and volume are both dependent on the quantity of matter observed
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Intensive property
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Where mass and volume are independent of amount of matter observed, aka the density is equal on both a glass of water and a pool
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Precision
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referrs to the degree of reproductivity of a measured quantity, that is closeness of agreement when the same quantity is measured several times
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Accuracy
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refers to how close a measured value is to accepted or actual value
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Law of Conservation of mass
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Lavoisier's law that the total mass of a substance present after a chemical reaction is the same as the total mass of substances before the reaction
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Law of Constant Composition(definite proportions)
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Proust's law that all samples of a compound have the same composition-the same proportions by mass of constituent elements
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Daltons Atomic Theory(3 points)
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1.Each element is made of indivisible particles called atoms
2. All atoms of a single element are alike in mass and other properties
3.In each of their compounds different elements combine in simple ratios
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Law of multiple proportions
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If two elements form more than a single compound, the masses of one element combined with a fixed mass of the second are in the ration of small whole numbers
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Cathode ray
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type of radiation emitted by negative terminal(cathode)
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Electrolysis
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the decompositon of a substance either in molten state or in an electrolyte solution, by means of electric current
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Protons
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positively charged fundamental particles of matter in nuclei of atoms
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Neutrons
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neutral particles
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Atomic number
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given number of protons in an atom
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Mass number
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total number of protons and neutrons in an atom
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Neutron number
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Mass number - proton number
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Isotopes
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atoms that have the same atomic number but different mass numbers
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Ions
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when atoms lose or gain electrons in the course of a chemical reaction, form ions, which carry net charges
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Molecular compound
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a small number of nonmetal atoms held together by covalent bonds
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Chemical formulas
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what represents molecular compounds which indicate the elements present and the relative number of atoms of each element
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empirical formula
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simplest formulas for compounds:shows types of atoms present and their relative numbers
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Molecular formula
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based on actual molecule of a compound
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Structural Formula
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shows the order in which atoms are bonded together in a molecule and by what types of bonds
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ionic compound
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compound made up of positive and negative ions joined together by electrostatic forces of attraction
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cation
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result of electron transfer that takes an electron away
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anion
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result of electron transfer that adds an electron, making to be negatively charged
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1 & 2 & 3 & 4
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mono & di & tri & tetra
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5 & 6 & 7 & 8 & 9 & 10
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penta & hexa & hepta & octa & nona & deca
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