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