CHEMISTRY first semester exam
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81 terms
Terms | Definitions |
|---|---|
 physical property | can be observed without changing a substance |
| chemical property | observed through a chemical change |
| extensive property (and two examples) | depend on amount, mass and volume |
| intensive property (and two examples) | independent of amount, density and boiling point |
| examples of chemical properties (2) | flammability, leaves changing due to photosynthesis |
| matter | anything that has mass and takes up space |
| element | same type of atom |
| compounds | atoms of different elements that are chemically combined |
| mixture | substances that are combined physically but have their own identities |
| heterogeneous mixture and one example | not the same throughout, can't see through it, mayonaise |
| homogeneous mixture and one example | same throughout, can see through it, salt water |
| direct relationship | y/x=k |
| indirect relationship | yx=k |
| formula for density | mass/volume |
| Avogadro's number | 6.022 X 10 ^23 |
| examples of chemical changes (3) | burning, rusting nail, combustion |
| examples of physical changes (3) | change in state, copper drawn into a wire, breaking glass |
| Law of Conservation of Mass | matter can neither be created nor destroyed in a normal chemical reaction |
| Law of Definite Proportions | ratio of elements is a whole number and is constant regardless of the amount of the sample |
| example of the Law of Definite Proportions | H2O (2:1) |
| Law of Multiple Proportions | elements may come together in different ratios to form different compounds |
| example of Law of Multiple Proportions | H2O and H2O2( water and hydrogen peroxide) |
| who created the atomic theory? | John Dalton (late 1800s) |
| five points of the atomic theory | matter is made of atoms, atoms of the same element are exactly alike, atoms are round solid and indivisable, law of definite proportions, chem reactions result from the rearrangement of atoms |
| what was Jj Thomson's experiment? | Cathode Ray Tube |
| What did J.J Thomson discover and what was his model? | electrons, Plum Pudding Model |
| Plum Pudding Model | pudding was the positive (protons) and plums were the negative electrons which were held together in the pudding |
| isotopes | atoms of the same element with a different number of neutrons |
| mass number | number of protons and neutrons |
| atomic number | number of protons |
| What was Rutherford's experiment? | Gold Foil Experiment |
| What were the three things that Rutherford deduced from his Gold Foil Experiment? | atom is mostly empty space, nucleus contains all the positive charge, electrons were outside nucleus (nothing about neutrons) |
| molar mass | mass of one mole of a pure substance |
| atomic mass | average mass of an element considering % natural abundance |
| how to calculate atomic mass (equation) | Amu weight X % abundance + 2nd Amu weight X % |
| which subatomic particle has the least mass? | electrons |
| all atoms of the same element have the same number of... | protons |
| planck's constant (h) | h= 6.626 X 10 ^ -34 |
| when are photons emitted/released? | electrons move to lower energy levels |
| ground state | lowest energy state when the electron is closest to the nucleus |
| nu | frequency |
| for a wave to have high energy it has | high frequency and low wave length |
| wave with low energy | low frequency and high wave length |
| lambda | wave length |
| amplitude | height of a wave |
| c/ speed of light | 3.00 X 10 ^8 m/s |
| formula for energy | Planck's constant X frequency |
| which has a higher energy : red or green light? | green |
| speed of light = (formula) | wavelength X frequency |
| what is the Schrodinger wave equation? | solved to find the probability of finding an electron in a region of space |
| The Pauli exclusion principle states that... | no two electrons from a given atom can have the same four quantum numbers |
| electronegativity increases.... | from left to right across the periodic table |
| principle quantum number | (n) size of the orbital, corresponds to energy levels (1-7) |
| Angular Momentum | (l) shape of the orbital, s p d f |
| magnetic quantum number | (m) describes axial orientation around the origin (x y z) |
| Hund's rule | electrons enter an orbital singly with like spin before going back to pair with opposite spins |
| valence electrons | outside electrons |
| inner shell/ core electrons correspond with what? | the noble gas that precedes it |
| Aufbau principle | electrons enter the lowest energy level sublevel combination first and completely fill it before beginning the next energy level sublevel combination |
| ionization energies | decrease down a group, increase across a period |
| linear (angle and polarity) | 180, non-polar |
| tetrahedral(angle and polarity) | 109.5, non-polar |
| trigonal pyramidal(angle and polarity) | 107, polar |
| bent (angle and polarity) | 104.5, polar |
| trigonal planar(angle and polarity) | 120, non polar |
| name the four types of crystals | metallic, ionic, network covalent, molecular |
| Boron and Aluminum are stable with how many electrons? | 6 |
| Beryllium is stable with how many electrons | 4 |
| isomer | same chemical formula with a different structure |
| hybridization | rearrangement of electrons during bonding |
| sp hybridization occurs when | all linear |
| sp2 hybridization occurs when? | trigonal planar, bent 120 |
| sp3 hybridization occurs when? | bent, tetrahedral, trigonal pyramidal |
| sp3d hybridization occurs when? | trigonal bipyramidal |
| sp3d2 occurs when? | octahedral |
| ionic crystal is between a ... and a ..... | metal and nonmetal |
| metallic | sea of electrons (between two metals) |
| ionic | transfer of electrons, forms crystal lattice structure |
| network covalent | 3D tetrahedral arrangement of atoms (diamonds and sand) |
| molecular occurs when.... | two nonmetals |
| Heisenberg Uncertainty Principle | it is impossible to calculate both the velocity and position of an electron in an atom simultaneously |
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