Chemistry Midterm Review – Flashcards
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| Mass |
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| Quantity of matter in an object SI base unit: kg |
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| volume |
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| space that an object occupies SI base unit: mL cm3 |
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| solid |
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| fixed volume and shape; particles vibrate |
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| liquid |
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| fixed volume but not shape; particles slip past each other. |
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| gas |
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| no fixed volume or shape. fastest moving particles |
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| 1 cm3 = |
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| 1 mL |
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| 1 dm3 = |
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| 1,000 mL or 1 L |
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| allotrope |
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| one of a number of different molecular forms of an element. such as; O2-oxygen and O3-ozone |
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| formula for density |
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| d=m/v |
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| 2 groups that make up pure substances |
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| elements and compounds |
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| law of conservation of energy |
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| Mass of product equals the mass of the reactants |
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| Law of Conservation of Energy |
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| The total quantity of energy remains constant. It cannot be created or destroyed. |
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| Kelvin to Celcius |
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| -273 |
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| Celcius to Kelvin |
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| +273 |
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| scientific method |
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| Specific procedures for conducting research -make/test hypothesis -observe -draw conclusions -publish results -construct theory |
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| theory |
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| a well-tested explanation of observations. Can be disproved but not fully proven |
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| hypothesis |
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| a reasonable and testable explanation for observations |
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| confined zeros |
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| significant |
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| leading zeros |
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| not significant |
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| trailing zeros following a decimal point |
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| significant |
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| qualitative |
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| describing something with properties such as texture and color used to describe quality |
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| quanttative |
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| describing something with numbers |
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| chemical change |
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| identity changes. new substance forms -evolution of gas -precipitate forms -release(exothermic) or absorption(endothermic) of energy -color change |
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| physical change |
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| identity does not change. can change state/mix but remain the original substance |
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| law of definite proportions |
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| two samples of a given compound are made of the same elements in the proportions by mass regardless of the sizes of sources of the samples |
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| law of multiple proportions |
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| if two or more different compounds are composed of the same elements, the ratio of mass in the second one is always a ratio of small whole numbers |
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| Daltons theory 1(revised) |
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| all matter is composed of extrememly small particles called atoms that cannot be subdivided or destroyed |
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| Daltons theory 2 (revised) |
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| Atoms of a given element are identical in their physical and chemical properties |
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| Daltons theory 3 |
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| Atoms of different elements differ in their physical and chemical properties |
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| Daltons theory 4 |
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| Atoms of different elements combine in simple, whole-number ratios to form compounds |
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| Daltons theory 5 |
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| In chemical reactions, atoms are combined, rearranged, or separated but NEVER created or destroyed. |
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| which subatomic particles reside in the nucleus? |
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| protons-positive neutrons- no charge |
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| subatomic particle outside the nucleus |
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| electrons- negative |
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| isotope |
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| Atoms of the same element with a different number of NEUTRONS |
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| ion |
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| an atom, radical or molecule that has gained or lost one or more electrons and now has a neg or pos charge |
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| what happens when an electron gains energy |
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| it moves into an excited state |
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| returning from an excited to ground |
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| it releases a specific quantity of energy and quickly falls back to its ground state |
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| Principal quantum number (n) |
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| indicates main level energy occupied by the electron ~1,2,3,4 |
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| Angular quantum number (l) |
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| indicates the shape or type of orbital that corresponds to a particular sublevel =0(s); =1(p); =2(d); =3(f) |
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| Magnetic Quantum Number (m) |
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| is a subset of the L quantum number. indicates the number/orientations around the nucleus 1-s orbital 3-p orbitals 5-d orbitals 7-f orbitals |
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| orbitals/electrons in s |
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| 1 orbital; 2 e- |
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| orbitals/electrons in p |
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| 3 orbitals; 6 electrons |
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| orbitals/electrons in d |
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| 5 orbitals; 10 e- |
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| orbitals/electrons in f |
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| 7 orbitals; 14 e- |
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| aufbau |
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| "building up" e- fill orbitals with lower energy first s>p>d>f |
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| Hund's |
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| orbitals of the same n and L quantum numbers are each occupied by one before paring occurs |
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| Pauli |
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| two particles of a certain class cannot be in the exact same energy state ^^ or vv |
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| Periodic Law |
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| The physical or chemical properties tend to repeat systematically with increasing atomic number |
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| 4f |
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| lanthanide |
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| 5f |
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| actinide |
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| 4f or 5f radioactive? |
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| 5f- actinides |
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| malleable |
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| can be hammered into a sheet and remain conductive |
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| ductie |
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| can be stretched into thin wire and remain conductive |
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| electron sheilding |
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| outer, valence e- held less tightly to nucleus |
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| down a group, e- shielding |
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| atomic radius increases down a group |
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| as the nuclear charge increases across a period |
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| the effective nuclear charge also increases |
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| ionization energy |
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| the amount of energy needed to remove an electron from an atom |
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| ionization energy -decreases -increases |
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| ionization energy -down a group -across a period |
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| electronegativity |
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| a measure of the ability of an atom in a chemical COMPOUND to attract electron |
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| electronegativity -decreases -increases |
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| electronegativity -down a group -across a period |
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| electron affinity |
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| the change in energy when a neutral atom gains an electron |
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| electron affinity -decreases -increases |
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| electron affinity -down a group -across a period |
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| ionic radii -increases -decreases |
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| ionic radii -down a group -across a period |
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| atomic radii -increases -decreases |
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| atomic radii -down a group -across a period |
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| group 1 |
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| 1+ |
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| group 2 |
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| 2+ |
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| group 15 |
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| 3- |
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| group 16 |
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| 2- |
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| anion |
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| ion with a negative charge |
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| cation |
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| an ion with a positive charge |
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| common between an ion and its parent atom |
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| proton count |
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| lattice energy |
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| the amount of energy released when an ionic bond is formed |
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| bond energy |
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| energy required to break the bond of 1 mole of a chemical compound |
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| properties of ionic compounds |
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| -hard and brittle -good conductors -strong -high boiling and melting points -solid at room temp |
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| for an ionic compound to conduct |
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| -substance must contain charged particles -must be free to move |
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| strongest attractive forces |
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| ionic |
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| why are ionic compounds considered brittle? |
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| when you apply a strong force, fracture occur, not dents |
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| CH3COO(1-) |
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| acetate |
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| S2O3(2-) |
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| thiosulfate |
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| NO2(1-) |
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| nitrite |
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| NO3(1-) |
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| nitrate |
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| PO4(3-) |
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| phosphate |
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| CO3(2-) |
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| Carbonate |
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| CN(1-) |
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| cyanide |
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| CrO4(2-) |
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| Chromate |
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| SO4(2-) |
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| Sulfate |
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| SO3(2-) |
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| Sulfite |
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| OH(1-) |
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| Hydroxide |
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| MnO4(1-) |
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| Permaganate |
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| Cr2O7(2-) |
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| Dichromate |
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| NH4(2-) |
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| Ammonium |
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| Covalent Bond stronger/weaker than ionic |
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| weaker than ionic |
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| weakest type of covalent bond |
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| nonpolar covalent |
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| tetrahedral atoms: bonds: |
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| tetrahedral 5 4 |
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| 0-0.5 |
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| nonpolar |
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| .6-2.0 |
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| polar covalent |
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| 2.1-4 |
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| ionic compound |
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| avogrados number |
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| 6.022x10^23 |
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| molar mass |
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| an average of the abundances of each weight of the element |
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| mass>particle |
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| mass given| 1 mol | avogrados# ..........|molar mass|1mol |
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| particle>mass |
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| Part. given| 1 mol | molar mass .........|avorgado#| 1 mol |
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| 1A |
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| alkali |
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| 2A |
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| alkaline earth |
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| 17A |
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| halogens |
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| 18 |
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| noble gases |
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| 3-12 |
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| transition metals (d block) |
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| which in d block break Aufbau to become more stable? |
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| Cromium and Copper |
