1. Chemistry – STAR Test Review – Day 1
Ch2 – Classifying Matter
1. Classify these as elements, compounds, or mixtures.
If mixture, decide if heterogeneous or homogeneous.
a. silver b. pine tree c. orange juice d. carbon dioxide e. air   
2. Classify each of the following changes as physical or chemical.
a. bread is baked b. salt dissolves in water
c. milk spoils d. A snowflake melts

2. Ch4,25 – The Atom and Nuclear Processes
1. What is the charge, positive or negative, of the nucleus of every atom?
2. Determine the number of neutrons in each atom.
a. nitrogen b. radium-226   
3. List the number of protons, neutrons, and electrons in each
of the following atoms.
a Al b Ca

3. 4. Tell how alpha, beta and gamma radiation are distinguished on the basis
of the following:
a. mass b. charge c. penetration power
5. Complete these nuclear reactions:   
a P  _____ e
b. _____  N e  

4. 6. Write nuclear reaction for the beta decay of the following isotope:
9038Sr
7. Write the nuclear reaction for this word equation:
a. Radon-222 emits an alpha particle to form polonium-218.

5. Ch5 – The Electron
___ Dalton a. planetary model of the atom, electrons move
around the nucleus like planets around sun
  ___ Bohr b. gold foil experiment – atoms have a dense core
called nucleus
  ___ Rutherford c. father of the modern atomic theory, everything
made of atoms
1. Find the Battleship Position, the Electron Configuration,
and the Orbital Filling Diagram for these atomic numbers:
a. Atomic number 15
b. Atomic number 56

6. 2. What is the frequency of radiation with a wavelength of 5
2. What is the frequency of radiation with a wavelength of 5.0 x 10-8 m?
3. What is the energy of a photon whose frequency is 3.0 x 1012 Hz?
Ch6 – Periodicity
1. Arrange these elements in order of decreasing atomic size:
sulfur, chlorine, aluminum and sodium.
Does your arrangement demonstrate a periodic or group trend?

7. 2. Distinguish between the first and second ionization energies of an atom.
3. Chlorine, selenium, and bromine are located near each other
on the period table. Which of these elements is the smallest atom?

8. 4. Which particle has the largest radius in each atom /ion pair?
a. Na, Na+ b. S, S-2
5. Why don’t the noble gases appear in an eletronegativity table?

9. Ch9 – Naming
1. Identify the following elements as metals, metalloids, or nonmetals.
a. gold b. silicon
2. The melting point of a compound is 1240’C, and ice melts at 0’C.
Is this compound an ionic or molecular compound?

10. 3. Write the formulas for these compounds.
a. barium fluoride b. calcium carbonate
c. lithium hypochlorite d. tin(II) hydroxide
e. tetraiodine nonoxide

11. 4. Write names for these compounds.
a. Al(OH)3 b. NaI
c. Sn3(PO4)2 d. CS2
e. Cl2O7 f. N2O5

12. Day 2
Ch10 – The Mole
1. How many moles are 2.80x1024 atoms of silicon?
2. Find the gram molecular mass of C3H7OH.   
3. What is the mass of 2.11 x 1024 molecules of sulfur dioxide?

13. 4. Find the volume at STP of 3.20 x 10-3 mol CO2 gas.
5. At STP, what volume does 12.2 g of fluorine gas occupy?
x 1024 molecules of argon occupy what volume at STP?

14. Ch11 – Chemical Reactions
1. Balance the following equations:
a. ___ PbO2  ___ PbO + ___ O2
b. ___ Li + ___ FeBr2  ___ LiBr + ___ Fe
c. ___ Al + ___ CuSO4  ___ Al2(SO4)3 + ___ Cu

15. 2. Rewrite these word equations as balanced chemical equations.
a. iron (III) chloride + calcium hydroxide 
iron (III) hydroxide + calcium chloride
b. sodium + water  sodium hydroxide + hydrogen

16. 3. Write the balanced chemical equation for the following
combination reaction:
Mg + O2 
4. Write the balanced chemical equation for the following
decomposition reaction:
HBr 
5. Write the balanced chemical equation for the following
single-replacement reaction:
Ag(s) + KNO3(aq) 

17. 6. Write a balanced chemical equation for the following
double replacement reactions:
HCl(aq) + Ca(OH)2(aq) 
7. After balancing the equation, identify the type.
a. ___ C2H6 + ___ O2  ___ CO2 + ___ H2O
b. ___ Pb(NO3)2 + ___ NaI  ___ PbI2 + ___ NaNO3

18. Ch12 – Stoichiometry
1. Determine the mass of lithium hydroxide produced when
0.38 g of lithium nitride reacts with water according
to the following equation:
Li3N + 3H2O → NH3 + 3LiOH

19. 2. Determine the mass of carbon dioxide produced when
0.85 g of butane reacts with oxygen according to the following equation:
2C4H O2 → 8CO2 + 10H2O
 3. ___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
Given 26 L O2, at STP, how many liters of CO2 will be produced?

20. 4. Carbon disulfide is an important industrial solvent.
It is prepared by the reaction of coke with sulfur dioxide.
5C + 2SO2  CS2 + 4CO
how many moles of CS2 form when 2.7 mol of C reacts?
 5. The reaction between fluorine with ammonia produces
dinitrogen tetrafluoride and hydrogen fluoride.
5F2(g) + 2NH3(g)  N2F4(g) + 6HF(g)
if you have 66.6 g of NH3, how many liters of F2
are required for complete reaction?