First Semester Final Exam - Review-1 Fall 2024.docx

Honors Chemistry 1st Semester Final Exam Review

Items that you have to know regardless of the unit:

  1. The 46 elements and their symbols covered at the beginning of the school year.
  2. The 33 polyatomic ions.
  3. Know the list of seven diatomic molecules

As always, remember to use and report answers to the correct significant figures and to include units!

FUNDAMENTALS OF CHEMISTRY: MATTER AND CHANGE (Ch 1 and 2)

  • Define chemistry.
  • 5 branches of chemistry
  • Which of the following observations is evidence used to imply that a chemical reaction has occurred?

a. gas evolution b. a precipitate forms c. the color changes

d. the temperature changes e. the odor changes f. a sound is produced

g. change in taste

  • Describe a physical property vs. a chemical property.
  • What is the difference between a physical change and a chemical change?
  • Identify each type of change (physical or chemical).

a. boiling water b. rusting iron c. burning candles

d. breaking glass e. melting wax

  • Be able to classify matter: mixtures (homogeneous, heterogeneous) vs. pure substances (compounds or elements)
  • What is an extensive property? An intensive property?
  • Identify each as an element, compound or mixture.

a. lead b. water c. kool-aid

d. table salt e. soda f. oxygen

  • What are the characteristic of a metal, metalloid and non-metal? Identify each type of element: a. Zn b. As c. S d. Ne e. Na

MEASUREMENTS AND CALCULATIONS (Ch 3)

  • Discuss the steps in the scientific method.
  • What are the rules/guidelines of determining significant figures?
  • How many significant figures in:

a. 1234 b. 123.0 c. 123400 d. 0.001234 e. 0.01230

  • Report the above problems (a-e) in correct scientific notation.
  • What are the common SI Units? Know the prefixes from milli to kilo and nano and be able to convert between units in the metric system.
  • What is the difference between mass and weight?
  • Multiply: 5.98 mm x 3.2 mm = ?
  • Add 3.258 cm + 12.0 cm = ?
  • Give an example of a qualitative observation
  • Give an example of a quantitative observation.
  • What is the difference between accuracy and precision?
  • How many grams of mercury would you have if you had 32 cm3 of mercury? The density of mercury is 13.6 g/cm3.
  • Ronnie has a piece of aluminum which has a mass of 10.8 grams and a volume of 4 cubic centimeters. Calculate the density of aluminum.

ATOMIC THEORY (chapter 4)

  • Describe Dalton’s Atomic Theory and the modern atomic theory.
  • What did we learn from Rutherford’s Gold Foil Experiment and how did it work?
  • What did J. J. Thomson discover with his Cathode Ray experiment?
  • Define the atomic number, mass number, average atomic mass and isotopes.
  • Explain the difference between atoms, ions, cations, anions.
  • Know the charge, location and size of the three subatomic particles.
  • Fill in the blanks for the following: 79 Br

137 Ba2+

37 Cl-

29Al

35 56 17

atomic number

mass number

# protons

# neutrons

# electrons

neutral or type of ion?

  • An element has 30 protons, 35 neutrons, and 30 electrons. What element is this?
  • An ion of an element has 29 protons, 35 neutrons, and 27 electrons. What ion is this? Write its symbol with the correct charge.
  • State the Law of Conservation of Mass (Matter).
  • Most of the volume of the atom is taken up by the electron cloud. True or False?
  • How do you calculate the relative atomic mass from percent abundances?
  • What instrument is used to find percent abundances in nature?

ELECTRON CONFIGURATIONS (Chapter 5)

  • What is the frequency of an electromagnetic wave traveling at the speed of light with a wavelength of 6.80 x 10-7 m?
  • All types of electromagnetic radiation have the same .
  • Identify the parts of an electromagnetic wave on a diagram (i.e. wavelength, amplitude, etc.).
  • What is a quantum of electromagnetic energy called?
  • Write the full electron configuration for: C, As, and S2-
  • How many outer electrons does each of the following have? Na As Br O2- K+
  • How many electrons must each of the following lose or gain to achieve an octet? (State whether it loses or gains and how many) Cl Ca Xe P
  • Which element has similar chemical properties like Si? Why? At Al N C
  • When electrons absorb energy, what is the result?
  • What color of light has the most energy?
  • What is the probability map for an electron called?
  • What is the principal quantum number? The magnetic quantum number?
  • What occurs when an electron moves from a higher energy level to a lower energy level in an atom?
  • The indicates the main energy level occupied by the electrons (n).
  • How many electrons can occupy an s orbital, p orbital, d and f orbitals?
  • How many total electrons are there in a p sublevel? p sublevel? s sublevel? f sublevel?
  • Which atom would have an octet of electrons (full s and p orbitals): Fe, Ar, O or He

PERIODIC TABLE (Ch 6)

  • Who is Dmitri Mendeleev? How did he organize the elements in the periodic table? How did he predict undiscovered elements.
  • How did Mosley organize the elements in the periodic table.
  • What charge do all elements in the following columns form when they are ions? 1, 2, 13, 15, 16, 17, 18
  • What is the chemical family name for column: 1, 2, 17 and 18?
  • What are the following groups most characteristic properties? 1, 2, 17, 18
  • Write the complete electron structure for a neutral sodium atom. According to its electron structure, what period of the periodic table should sodium be in? How many valence electrons does it have? What ion will sodium tend to form?
  • What is meant by a noble gas electron configuration? Why are they more stable?
  • Define: electronegativity ionization energy electron affinity Atomic radius
  • Describe the trends (across a period, down a group) in the periodic table for: Atomic radius Ionization energy Electronegativity
  • State the periodic law.

IONIC COMPOUNDS (Ch 7 & 8)

  • Use the following ions and write the correct formula for the compound made from them:

a. Na+ and Br- b. Mg2+ and I- c. Ca2+ and NO - d. Fe3+ and SO 2-

3 4

  • Name the above compounds (a-d) and the following: e. KOH f. CuF g. CuSO4
  • Which compounds below are ionic? Which are molecular (covalently bonded)?

a. N2 b. CaF2 c. NO2 d. CuSO4 e. CCl4

  • Given SO 2- and the compound Zr (SO ) , what is the charge on Zirconium?

4 2 4 3

  • What is the chemical formula for potassium chlorite? What is the formula for iron(III) sulfide?
  • What is the formula for lithium carbonate?
  • Properties of ionic compounds
  • Properties of metals
  • Metallic bonds and alloys

COVALENT COMPOUNDS (Ch 7 and 9)

  • What is a chemical bond?
  • What are valence electrons and why are they important?
  • State the octet rule.
  • What is the difference between ionic, covalent and metallic bonding?
  • What type of bond (ionic or covalent) will form in the following compounds? How do you know? CO2 NaCl F2
  • What is the charge of an Oxygen ion? Nitrogen? Calcium? Sodium?
  • Using an electronegativity chart identify each type of bonding (ionic, polar covalent, nonpolar covalent): Cs – Cl H – O Br – I Cl – Cl
  • What are all the exceptions to the octect rule?
  • What is VSEPR theory?
  • Draw Lewis dot structure and predict geometry and shape.
  • Use VSEPR theory to predict the molecular geometry and polarity of the following molecules: CO2 CH4 BF3 H2O SF6 PCl5 NH3
  • What is the formula for Phosphoric acid? For Hydrophosphoric acid?
  • Name each of the following acids: a. HCl b H2SO4 c. HNO3 d. HI