Question | Answer |
Matter | Anything that has mass and takes up space |
States of matter | Solid, liquid, gas |
Physical properties | All properties that do not involve chemical reactions |
Chemical properties | The chemical reactions a substance undergoes |
Chemical change/Chemical reaction | Substances are used up (disappear) and others are formed to take their places |
Physical changes | Change where the identity of the substances do not change; most involve changes of state |
Calculation for density | d=m/v |
Calculation for specific gravity | Density in g/mL / 1.00 g/mL (it is unitless/dimensionless) |
Classifications of matter | Matter -> pure substances and mixtures. Pure substances can be divided into elements, which chemically combine to form compounds. Mixtures can be divided into homogenous and heterogenous matter. |
Diatomic elements | O2, H2, N2, F2, Cl2, Br2, I2 |
Three subatomic particles of an atom | Proton, electron, neutron |
Proton | A subatomic particle that has a positive charge (+1) and a mass of approximately 1 amu; it is found in a nucleus |
Electron | A subatomic particle with a charge of -1 and a mass of approximately 0.0005 amu. It is found in the space surrounding a nucleus |
Neutron | A subatomic particle with a mass of approximately 1 amu and a charge of zero; found in the nucleus |
Mass number | The sum of the number of protons and neutrons in an atoms nucleus |
Atomic number | Number of protons in an atoms nucleus |
Isotopes | Atoms with the same number of protons but different numbers of neutrons |
Atomic weight | The weighted average of the masses of the naturally occurring isotopes of the element. The units are amus |
Periods and groups | 7 periods and 18 groups |
Hydrogen | H |
Lithium | Li |
Sodium | Na |
Potassium | K |
Rubidium | Rb |
Cesium | Cs |
Francium | Fr |
Beryllium | Be |
Magnesium | Mg |
Calcium | Ca |
Strontium | Sr |
Barium | Ba |
Radium | Ra |
Fluorine | F |
Chlorine | Cl |
Bromine | Br |
Iodine | I |
Astatine | At |
Helium | He |
Neon | Ne |
Argon | Ar |
Kr | Krypton |
Xenon | Xe |
Radon | Rn |
Ununoctium | Uuo |
Manganese | Mn |
Iron | Fe |
Cobalt | Co |
Copper | Cu |
Silver | Ag |
Lead | Pb |
Tin | Sn |
Ground state electron configuration | The lowest possible energy level of an atom |
How many "s" orbitals are there | 1 |
How many "p" orbitals are there | 3 |
How many "d" orbitals are there | 5 |
How many "f" orbitals are there | 7 |
Argons electron configuration (18) | 1s2 2s2 2p6 3s2 3p6 |
Valence shell | Outermost occupied shell of an atom |
Valence electron | An electron in the outermost occupied shell of an atom |
Ionization energy | Increases as you go up and to the right; the energy required to remove the most loosely held electron from an atom in the gas phase |
Anion | An ion with a negative electric charge |
Cation | An ion with a positive electric charge |
Octet rule | When undergoing chemical reaction, atoms of group 1A-7A elements (main group elements) tend to gain, lose, or share sufficient electrons to achieve an election configuration having eight valence electrons |
Ammonium | NH4+ |
Hydroxide | OH- |
Nitrite | NO2- |
Nitrate | NO3- |
Acetate | CH3COO- |
Cyanide | CN- |
Permanganate | MnO4- |
Chromate | CrO4^2- |
Dichromate | Cr2O7^2- |
Hydrogen carbonate | HCO3- |
Sulfite | SO3^2- |
Hydrogen sulfite | HSO3- |
Sulfate | SO4^2- |
Hydrogen sulfate | HSO4- |
Phosphate | PO4^3- |
Hydrogen phosphate | HPO4^2- |
Dihydrogen phosphate | H2PO4- |
Maximum number of electrons in each orbital | Two |
Shell 1 | One 1s orbital, can hold 2 electrons |
Shell 2 | One 2s and three 2p orbitals, can hold eight electrons |
Shell 3 | One 3s, three 3p, and 5 3d orbitals, can hold 18 electrons |
Atomic radius trends | For main group elements, atomic radii increase going down a group and decrease going from left to right across a period |
Ionic bond | A chemical bond resulting from the attrition between positive and negative ions (metal and non-metal) |
Covalent bond | A chemical bond resulting from the sharing of electrons between two atoms (two non-metals) |
Nonpolar covalent bond | A covalent bond between two atoms whose difference in electronegativity is less than 0.5 |
Polar covalent bond | A covalent bond between two atoms whose difference in electronegativity is between 0.5 and 1.9 |
Ionic bond | A bond whose difference in electronegativity is greater than 1.9 |
Single bond | A bond formed by sharing one pair of electrons and represented by a single line between two atoms |
Double bond | A bond formed by sharing two pairs of electrons and represented by two lines between the two bonded atoms |
Triple bond | A bond formed by sharing three pairs of electrons and represented by three lines between the two bonded atoms |
Geometry of an atom surrounded by two groups | Linear |
Geometry of an atom surrounded by three groups | Trigonal planar |
Geometry of an atom surrounded by four groups with four covalent bonds | Tetrahedral |
Geometry of an atom surrounded by four groups with three covalent bonds | Tetrahedral Trigonal pyramidal |
Geometry of an atom surrounded by four groups with two covalent bonds | Tetrahedral Bent |
Bonds can be polar but depending upon the geometry of the molecule, they can be non polar | |