Final Exam Review-1

Page 1: Definitions and Concepts

Definitions of Key Terms

  • Atomic Sizea. Inner electrons of an atom not involved in bonding

  • Bond Energyb. Energy released in the form of light

  • Bonding Pairsc. Pair of electrons shared between two atoms

  • Chemical Bondi. Forces that hold molecules together

  • Core Electronse. Electrons in the lowest energy shells not involved in bonding

  • Covalent Bondo. Chemical bond that results from sharing electrons

  • Covalent Compoundb. Compound made of 2 or more nonmetals

  • Dipole Momentl. Molecule with a charge distribution (a positive and negative center)

  • Duet Rulec. Hydrogen and helium preference for having 2 valence electrons

  • Electron Configurationj. Arrangement of electrons around the nucleus of an atom

  • Electronegativityf. Ability of an atom in a molecule to attract shared electrons to itself

  • Emissiond. Energy released in the form of light

  • Excited Statek. Atom with excess energy

  • Frequencyg. # of waves per time period that pass a given point in space

  • Ground Stateh. Atom in the lowest possible energy state

  • Ionic Bondh. Chemical bond that results from transfer of electrons

  • Ionic Compoundf. Compound made of a metal and a nonmetal

  • Ionization Energyj. Energy required to remove an electron from an atom

  • Lewis Structurea. Shows how valence electrons are arranged around atoms

  • Lone Pairso. Pairs of electrons that are unshared

  • Nonpolar Compoundb. Compound with a net dipole of zero

  • Octet Rulei. Atom's preference for having 8 valence electrons

  • Orbital Diagramn. Pictorial representation of an atom’s electron distribution and spin

  • Photonc. A particle of light or quantum of electromagnetic energy

  • Polar Covalent Bondg. A bond that results from an unequal sharing of electrons

  • Polar Compoundm. A compound with an overall net dipole

  • Quantizedk. Energy levels exist in discrete, non-continuous energy levels

  • Speed of Lightd. 2.9979 x 108 m/s

  • Valence Electronse. Outermost electrons of an atom involved in bonding

  • Wavelengthl. Distance between successive peaks in a wave

Electron Configurations

  1. Write the electron configurations for the following elements:

  • Sulfur

  • Sodium

  • Neon

  • Chlorine

Page 2: Electron Configuration and Trends

  • Identify Elements from Electron Configuration

    • 1s²2s²2p⁶

    • 1s²2s²2p⁶ 3s²3p⁶ 4s¹

Ranking Periodic Trends

  • Atomic Size (largest to smallest)

    • Cs, Fr, Li, Na

  • Electronegativity (largest to smallest)

    • Li, Na, Cs, Fr

  • Ionization Energy (largest to smallest)

    • F, C, B, Be

Valence Electrons and Ion Charge

  • Li - 1 valence electron, charge of ion: +1

  • N - 5 valence electrons, charge of ion: -3

  • F - 7 valence electrons, charge of ion: -1

  • S - 6 valence electrons, charge of ion: -2

Drawing Lewis Structures

  1. CCl4

  2. CO

  3. H2O

Page 3: Gas Law Calculations

Gas Law Problems

  1. Given: Volume = 5,000 L, Pressure = 1.08 atm, Moles = 301. Find Temperature.

  2. Given: Volume = 859 L at 1.2 atm, find new volume at 2.8 atm.

  3. Balloon problem: Volume at 34.8°C and 0.97 atm, new volume when temperature is 21.0°C and pressure drops to 0.71 atm.

  4. Calculate volume change of a balloon dropped into liquid nitrogen (from 25.4°C to -196°C).

Page 4: Gas Laws and Chemical Calculations

Total Pressure Calculation

  1. Total Pressure of air composed of:

  • N2: 0.81 atm

  • O2: 0.19 atm

  • CO2: 0.05 atm

  • H2O: 0.02 atm

Volume of Oxygen Gas Production

  1. Find volume of oxygen gas produced at 1.32 atm and 30°C from 20 grams of potassium chlorate.

Balancing Chemical Equations

  1. Balance the following equations:

  • Fe + Cl₂ → FeCl₃

  • KMnO4 + HCl → KCl + HMnO4

  • C6H5COOH + O2 → CO2 + H2O

Molar Mass Calculation

  1. Calculate the molar mass of B2(PO4)3.

  2. How many grams in 1.89 moles of B2(PO4)3?

Page 5: Moles and Chemical Reactions

Moles of Compounds

  1. How many moles in 1154 grams of B2(PO4)3?How many molecules in 875 moles of B2(PO4)3?

  2. How many moles in 3.81 x 10¹⁹ molecules of B2(PO4)3?

Writing Chemical Equations

  1. Write the chemical equation for:

  • Sodium chloride + Iron(III) nitrate results in iron(III) chloride + sodium nitrate.

Sentence Conversion of Chemical Reactions

  1. Convert the chemical equation Sr(NO3)2 + 2 NaOH → Sr(OH)2 + 2 NaNO3 into a sentence.

Page 6: Chemical Reactions and Yields

Combustion Reaction and Yields

  1. Based on the equation:

  • 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

  • a. Limiting reagent and theoretical yield from given masses of C8H18 and O2.

  • b. Calculate % yield for CO2 (145 grams produced) and H2O (50 grams produced).

Molar Masses for Calculations

  • Molar masses:

    • C8H18 = 114 g/mol

    • O2 = 32 g/mol

    • CO2 = 44 g/mol

    • H2O = 18 g/mol