Chem Final Review
Unit 1 - Matter and Atomic Structure
Mixtures
Homogenous: composition is the same in proportion throughout (salt water)
Heterogenous: composition is different in proportion throughout (stew)
Elemental: only consisting of one element (O2, Ar)
Compound: consisting of two or more elements
Molecules: consisting of two or more atoms (O2, CH4)
Atoms: consisting of one atom (Au)
Density = m/v
Periodic Table
Atomic number: top number on the element, equal to the number of protons
Number of protons: top number on the element, equal to the atomic number
Electrons: equal to the number of protons if not an ion, otherwise determined by the charge
Neutrons: atomic mass (bottom of the element) - protons
Atomic mass: number on the bottom of the element or listed like Titanium-47
Finding the abundance
Symbol | Mass | % Abundance |
Li-6 | 6.015122 | 7.590 |
Li-7 | 7.016004 | 92.41 |
(6.015122 .07590) + (7.016004 .9241) =6.940 amu
Unit 2 - Light and Electron Configuration
Light
Wavelength and frequency are inversely related, the smaller the wavelength, the higher the frequency
The atom absorbs energy, causing the electrons to move from a ground state (closer to the nucleus) to an excited state (farther from the nucleus). When the electron returns the atom releases the energy it absorbed in the form of a photon
Electron Configurations
Begins as 1s22s22p63s23p64s23d104p6… goes to 4th P level then to 3d and from A56 to A57 (6s2 to 4f)
S-2 P-6 D-10 F-14
Oxide ion has -2 (aligning it with the noble gas)
Carbide ion has -4 (aligning it with the noble gas)
Unit 3 - Periodic Table and Trends
Trends
Atomic Radius: ⬇⬅ (Francium biggest) Atomic radius decreases across a period (row) since effective charge increases along a period, causing the attraction to be higher and making the electron cloud smaller.
Ionic Radius: ⬇⬅ (Francium biggest)
Ionization Energy/Energy required to remove an electron: ⬆➡ (Helium highest) Ionization energy is higher across a period since the effective nuclear charge is higher, making removing it more difficult. Ionization decreases down a group (is easier to remove) since energy levels increase and therefore the balance electrons are further apart and less attracted to the nucleus.
Electronegativity/Ability to attract electrons: ⬆➡ (Fluorine highest) Electronegativity increases across a period (row) since the effective nuclear charge increases across a row. It decreases down a group since energy levels increase down a group and make valence electrons further from the nucleus, therefore making attraction more difficult.
Metals vs Nonmetals
Metals: malleable, high melting point, low electronegativities, low ionization energy, metals lose electrons
Non-metals: non-malleable, varying melting points, higher electronegativities/ionization energy, non-metals gain electrons
Unit 4 - Bonding
Lewis Structures
Trigonal Planar | 3 electron domains (3 bonding, 0 non-bonding) | |
Linear | 2 electron domains (2 bonding, 0 non-bonding) | |
Tetrahedral | 4 electron domains (4 bonding, 0 non-bonding) | |
Pyramidal | 4 electron domains (3 bonding, 1 non-bonding) | |
Bent | 4 electron domains (2 bonding, 1 non-bonding) | |
Bent | 4 electron domains (2 bonding, 2 non-bonding) |
Bonds
Ionic: Metal and Non-metal, electrons are transferred from metal to the non-metal
Soluble and conductive
Polar Covalent: Non-metal and Non-metal with different electronegativities, electrons are shared unequally
Soluble but not conductive
Non-polar Covalent: Non-metal and Non-metal with similar or the same electronegativity, electrons are shared equally
All no: Doesn’t dissolve in water or conduct electricity. Not malleable.
Metallic: Metal and Metal: None want the electrons, creating a sea of electrons creating an electrical current and conducting electricity
Conducts electricity in bulk phase, is malleable.
Polyatomic ions can have both covalent and ionic bonding. Ionic between the counterion and polyatomic ion, covalent between the atoms within the polyatomic ions.
Unit 5 - Nomenclature
Naming
Transition metal: include the charge in name
Non-metals: include a prefix, always on second, on first if not “one”
The second element gets an ide (not polyatomic ion)
Polyatomic ions leave as is
Unit 6 - Moles and Empirical Molecular Formulas
Empirical/Molecular Formulas
Put percent as a mass
Convert mass to moles
Divide by the smallest mole number
Multiply until whole number
To make it molecular take the empirical formula and add up the mass and then if not the mass multiply until it is
Unit 7 - Balancing Reactions and Predicting Products
Combustion produces CO2 and H2O
Double Replacement reactions occur if a precipitate is formed
For Single Replacement reactions to occur, the metal must be higher on the activity series than the one it is trying to replace
Unit 8 - Stoichiometry
Use a molar ratio
Whichever makes the least product (solve for the same one) is the limiting reactant
Percent yield = actual yield/theoretical yield x 100
When calculating what will be produced (product), multiply
When calculating what needs to occur for something to be produced (reactant), divide
Unit 9 - Gases
PV=nRT
PV/NT=PV/NT
Divide = direct, Multiply = Inverse
Add 273 to Celsius
Unit 10 - Solutions
Molarity = mol of solute/liters of solution
Ensure convert to liters (and grams to moles)
MV=MV
Saturated = can’t add any more
Unsaturated = can add more
Unit 11 - Acids and Bases
Acids
Source of H+ (ex: HCl, H2SO4
Ionic bonding (soluble and conductive, categorized as an electrolyte)
pH under 7
Sour
Turns clear
Neutralize with baking soda (a weak base)
Bases
Source of OH- (NaOH, KOH)
Ionic bonding (soluble and conductive, categorized as an electrolyte)
pH over 7
Bitter
Turns pink
Neutralize with vinegar (a weak acid)
A specific kind of double replacement reaction
Acid + Base -> Salt (Conjugate Base) + Water (Conjugate Acid)
In a Bronsted-Lowry reaction, protons are transferred
Bases accept H+ ions
Acids donate H+ ions
Strong acids completely dissociate, weak acids do not
If it is an ionic bond (metal and non-metal) or contains a polyatomic ion it is an electrolyte
Unit 1 - Matter and Atomic Structure
Mixtures
Homogenous: composition is the same in proportion throughout (salt water)
Heterogenous: composition is different in proportion throughout (stew)
Elemental: only consisting of one element (O2, Ar)
Compound: consisting of two or more elements
Molecules: consisting of two or more atoms (O2, CH4)
Atoms: consisting of one atom (Au)
Density = m/v
Periodic Table
Atomic number: top number on the element, equal to the number of protons
Number of protons: top number on the element, equal to the atomic number
Electrons: equal to the number of protons if not an ion, otherwise determined by the charge
Neutrons: atomic mass (bottom of the element) - protons
Atomic mass: number on the bottom of the element or listed like Titanium-47
Finding the abundance
Symbol | Mass | % Abundance |
Li-6 | 6.015122 | 7.590 |
Li-7 | 7.016004 | 92.41 |
(6.015122 .07590) + (7.016004 .9241) =6.940 amu
Unit 2 - Light and Electron Configuration
Light
Wavelength and frequency are inversely related, the smaller the wavelength, the higher the frequency
The atom absorbs energy, causing the electrons to move from a ground state (closer to the nucleus) to an excited state (farther from the nucleus). When the electron returns the atom releases the energy it absorbed in the form of a photon
Electron Configurations
Begins as 1s22s22p63s23p64s23d104p6… goes to 4th P level then to 3d and from A56 to A57 (6s2 to 4f)
S-2 P-6 D-10 F-14
Oxide ion has -2 (aligning it with the noble gas)
Carbide ion has -4 (aligning it with the noble gas)
Unit 3 - Periodic Table and Trends
Trends
Atomic Radius: ⬇⬅ (Francium biggest) Atomic radius decreases across a period (row) since effective charge increases along a period, causing the attraction to be higher and making the electron cloud smaller.
Ionic Radius: ⬇⬅ (Francium biggest)
Ionization Energy/Energy required to remove an electron: ⬆➡ (Helium highest) Ionization energy is higher across a period since the effective nuclear charge is higher, making removing it more difficult. Ionization decreases down a group (is easier to remove) since energy levels increase and therefore the balance electrons are further apart and less attracted to the nucleus.
Electronegativity/Ability to attract electrons: ⬆➡ (Fluorine highest) Electronegativity increases across a period (row) since the effective nuclear charge increases across a row. It decreases down a group since energy levels increase down a group and make valence electrons further from the nucleus, therefore making attraction more difficult.
Metals vs Nonmetals
Metals: malleable, high melting point, low electronegativities, low ionization energy, metals lose electrons
Non-metals: non-malleable, varying melting points, higher electronegativities/ionization energy, non-metals gain electrons
Unit 4 - Bonding
Lewis Structures
Trigonal Planar | 3 electron domains (3 bonding, 0 non-bonding) | |
Linear | 2 electron domains (2 bonding, 0 non-bonding) | |
Tetrahedral | 4 electron domains (4 bonding, 0 non-bonding) | |
Pyramidal | 4 electron domains (3 bonding, 1 non-bonding) | |
Bent | 4 electron domains (2 bonding, 1 non-bonding) | |
Bent | 4 electron domains (2 bonding, 2 non-bonding) |
Bonds
Ionic: Metal and Non-metal, electrons are transferred from metal to the non-metal
Soluble and conductive
Polar Covalent: Non-metal and Non-metal with different electronegativities, electrons are shared unequally
Soluble but not conductive
Non-polar Covalent: Non-metal and Non-metal with similar or the same electronegativity, electrons are shared equally
All no: Doesn’t dissolve in water or conduct electricity. Not malleable.
Metallic: Metal and Metal: None want the electrons, creating a sea of electrons creating an electrical current and conducting electricity
Conducts electricity in bulk phase, is malleable.
Polyatomic ions can have both covalent and ionic bonding. Ionic between the counterion and polyatomic ion, covalent between the atoms within the polyatomic ions.
Unit 5 - Nomenclature
Naming
Transition metal: include the charge in name
Non-metals: include a prefix, always on second, on first if not “one”
The second element gets an ide (not polyatomic ion)
Polyatomic ions leave as is
Unit 6 - Moles and Empirical Molecular Formulas
Empirical/Molecular Formulas
Put percent as a mass
Convert mass to moles
Divide by the smallest mole number
Multiply until whole number
To make it molecular take the empirical formula and add up the mass and then if not the mass multiply until it is
Unit 7 - Balancing Reactions and Predicting Products
Combustion produces CO2 and H2O
Double Replacement reactions occur if a precipitate is formed
For Single Replacement reactions to occur, the metal must be higher on the activity series than the one it is trying to replace
Unit 8 - Stoichiometry
Use a molar ratio
Whichever makes the least product (solve for the same one) is the limiting reactant
Percent yield = actual yield/theoretical yield x 100
When calculating what will be produced (product), multiply
When calculating what needs to occur for something to be produced (reactant), divide
Unit 9 - Gases
PV=nRT
PV/NT=PV/NT
Divide = direct, Multiply = Inverse
Add 273 to Celsius
Unit 10 - Solutions
Molarity = mol of solute/liters of solution
Ensure convert to liters (and grams to moles)
MV=MV
Saturated = can’t add any more
Unsaturated = can add more
Unit 11 - Acids and Bases
Acids
Source of H+ (ex: HCl, H2SO4
Ionic bonding (soluble and conductive, categorized as an electrolyte)
pH under 7
Sour
Turns clear
Neutralize with baking soda (a weak base)
Bases
Source of OH- (NaOH, KOH)
Ionic bonding (soluble and conductive, categorized as an electrolyte)
pH over 7
Bitter
Turns pink
Neutralize with vinegar (a weak acid)
A specific kind of double replacement reaction
Acid + Base -> Salt (Conjugate Base) + Water (Conjugate Acid)
In a Bronsted-Lowry reaction, protons are transferred
Bases accept H+ ions
Acids donate H+ ions
Strong acids completely dissociate, weak acids do not
If it is an ionic bond (metal and non-metal) or contains a polyatomic ion it is an electrolyte