Chemistry Exam – Flashcards
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| Name all the prefixes in the metric system in increasing order. |
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| Mili, Centi, Deci, Deca, Hecto, Kilo |
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| Scientific Notation |
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| A method of writing or displaying numbers in terms of a decimal number between 1 and 10 multiplied by a power of 10. |
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| Density Formula |
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| Density= Mass divided by volume |
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| List the physical properties of a substance. |
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| -Color -Smell -Brittle -Density -Melting Point -Boiling Point |
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| List chemical properties of a substance: |
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| -Flammability -Rusting -PH -Reactivity with acid |
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| What is a homogeneous mixture? |
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| Appears the same throughout |
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| Give examples of homogeneous mixtures: |
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| Water, air, milk, steel |
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| What is a heterogeneous mixture? |
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| Does not look the same throughout. |
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| Name some examples of a heterogeneous mixture |
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| Cereal, oil and water, Sand |
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| How would you separate homogeneous mixture like alcohol and water? |
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| Distilation |
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| How can you separate a compound and a mixture? |
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| By chemical means |
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| What is the difference between a compound and a mixture? |
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| Compound Cannot be easily separated |
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| How do you write a chemical symbol? |
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| The first letter is capitalized. |
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| List the steps to separate a mixture of water, salt, and iron filings. |
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| 1)Use magnet to remove iron 2)Boil water, collect salt crystals |
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| 3 Phases of Matter |
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| -Solid -Liquid -Gas |
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| Which phase takes the shape of its container and has a definate volume? Which has its own shape? |
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| Liquid takes the shape of its caontainer, solid has its own shape. |
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| Give 2 examples of a chemical change. |
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| -Rust -Burning |
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| Give 2 examples of a physical change. |
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| -Break -Crack |
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| Law of Conservation of Matter |
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| Matter can't be created or destroyed. It can only be transformed |
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| Law of Conservation of Energy state |
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| Energy is never created or destroyed only converted. |
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| Atom |
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| The basic unit of a chemical element |
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| Who named the atom? |
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| Democrates |
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| Element |
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| A substance that cannot be broken down by chemical means, defined by the number of protons they possess. |
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| Nucleus |
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| The positively charged central core of an atom, containing most of its mass. |
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| Proton |
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| A stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal to an electron. |
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| Neutron |
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| A subatomic particle of about the same mass as a proton but without an electric charge. |
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| Electron |
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| A stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity |
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| Ion |
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| An atom or molecule with a net electric charge due to the loss or gain of one or more electrons. |
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| Isotope |
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| Element that contains equal numbers of protons but different numbers of neutrons. |
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| Valance Electrons |
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| An electron in the outer shell of an atom which can combine with other atoms to form molecules. |
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| Orbital Diagrams |
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| Diagrams used to show how the orbitals of a subshell are occupied by electrons |
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| Ground State |
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| The lowest energy state of an atom or other particle. |
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| Excited State |
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| A state of a physical system that is higher in energy than the ground state. |
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| What is the atomic number equal to? |
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| The number of protons. |
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| What is the atomic mass or mass number equal to? |
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| The number of electrons. |
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| What particle changes in an atom with an increase in atomic number? |
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| The number of protons. |
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| How do you find the number of neutrons in an atom? |
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| Subtract the atomic number from the atomic mass. |
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| What must happen to change an atom from an atom into an ion? |
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| It must be oxidized. |
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| What particle changes in an atom to make it an isotope? |
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| The number of neutrons changes. |
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| Why are atomic masses written in decimal form on the periodic table? |
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| They are the average of all masses. |
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| Explain the steps to the flame test and how light was created in the flame test. |
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| Different chemicals created different colors of light. |
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| How do electrons move up and down energy levels? |
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| They get into an excited state and jump levels. |
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| Periodic Law |
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| The principle that chemical properties of the elements are periodic functions of their atomic numbers. |
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| Periodic Table |
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| A table of the chemical elements arranged in order of atomic number. |
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| Metal |
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| A solid material that is typically hard, and shiny with good electrical and thermal conductivity. |
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| Nonmetal |
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| Chemical elements that form negative ions, have acidic oxides, and are generally poor conductors of heat and electricity |
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| Metalloid |
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| An element whose properties are intermediate between those of metals and solid nonmetals |
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| Ionization Energy |
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| The energy required to remove an electron from an ion. |
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| What is a period on the Periodic Table and how many are there? |
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| Horizontal rows in the Periodic Table. There are seven. |
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| How does the size of an atom vary as you go across a period? |
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| The atomic radius decreases |
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| How does the Ionization energy vary as you go across a period? |
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| It increases. |
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| What is a family or group on the Periodic Table? |
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| The vertical columns on the Periodic Table. |
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| What happens to the size of atoms as you go down a family? |
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| It increases. |
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| What happens to the ionization energy as you go down a family? |
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| It decreases. |
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| Why are valence electrons so important? |
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| Tells how an element will react. |
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| What are the characteristics of metals? |
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| Good conductors of electricity and heat, shiny, lose electrons, high melting point. |
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| What are the characteristics of a nonmetal? |
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| Not good conductors, not shiny |
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| Where are nonmetals located on the periodic table? |
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| The top right of the table. |
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| What are the 7 metalloids, and where are they located? |
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| Boron-Family 13 Carbon-Family 14 Nitrogen-Family 15 Oxygen-Family 16 Fluorine-Family 17 |
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| Ionic Bond |
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| A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion |
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| Covalent Bonding |
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| A chemical bond that involves sharing a pair of electrons between atoms in a molecule. |
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| Octet Rule |
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| States that elements in the second row of the periodic table cannot have more than eight valence electrons around them them, whether as non-bonding electrons or in chemical bonds. |
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| What kinds of elements make up an ionic bond? |
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| Nonmetals and Metals |
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| What is happening in a covalent bond? |
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| Electrons are shared |
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| What types of elements are bonded together in a covalent bond? |
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| All nonmetals. |
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| How do you determine what a charge on an atom will be? |
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| When does an atom gain electrons and when does it lose electrons? |
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| Alkane |
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| Chemical compounds that consist only of hydrogen and carbon atoms and are bonded exclusively by single bonds |
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| Alkene |
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| Unsaturated hydrocarbons that contain at least one double bond. |
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| Alkyl groups |
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| Chemical compounds that consist only of hydrogen and carbon atoms and are bonded exclusively by single bonds |
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| Organic Chemistry |
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| The study of the thousands of carbon, containing the compounds. |
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| Alkyne |
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| Hydrocarbons with a triple bond. |
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| Name the first 10 prefixes used for carbon compounds. |
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| Mono, Di Tri, Tetra, Penta, Hexa, Hepta, Octa, Nona, Deca. |
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| When do you use the endings -ene and -yne? |
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| -ene One double, 2 singles -yne One double, 2 triples |
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| Lewis Dot Structure |
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| shows the bonding between atoms of a molecule. |
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| Electronegativity |
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| The tendency of an atom or to attract electrons to itself. |
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| Atomic Radius |
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| Distance from the nucleus of the atom to the outermost level. |
