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CHEM 1010 Test 1
Chapters 1-3
| 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 |
Created by:
AliRutherford
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