CP Chemistry Midterm REVIEW GUIDE Units 1-6
(do on another piece of paper)
____
1. Which of the following is a chemical change?
____
2. The diameter of a sulfur atom is 0.000 000 00 293 L. What is this number expressed in
scientific notation? 2.93 x 10- 9
____
3. How many significant figures are in the measurement 361.98 grams? 5
____
4. What is the measurement 2039 L rounded off to three significant digits? 204 L
____
5. What is the temperature of absolute zero measured in C? -273 degrees C ( 0 K)
____
6. All atoms of the same element have the same ____.
____
7. Which of the following sets of symbols represents isotopes of the same element?
a.
c.
C
C
C
E
E
E
a.
b.
a.
b.
b.
Evaporation
Freezing
number of neutrons
number of protons
H
H
c.
d.
c.
d.
d.
H
rusting
Boiling
mass numbers
mass
M
M
M
____
8. Who arranged the elements according to atomic mass and used the arrangement to predict
the properties of missing elements? (KNOW YOUR SCIENTITSTS!!!)
____
9. In looking at the periodic table, which are there more of? Metals or Nonmetals?
____ 10. Of the elements Ti, Ag, K, and He, which is a nonmetal?
____ 11. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p, 4s? 3d
____ 12. What is the number of electrons in the outermost energy level of a nitrogen atom? 5
____ 13. What is the electron configuration of calcium? 1s2 2s2 2p6 3s2 3p6 4s2
____ 14. How many electrons does fluorine gain in order to achieve a noble-gas electron
configuration? one
____ 15. Know the difference between an ionic bond and a covalent bond. Ionic- transferred
electrons; covalent—shared electrons
____ 16. What is the shape of the water molecule? What is the shape of CO2? Water- bent; Co2 linear
____ 17. Which atom in a water molecule has the greatest electronegativity? (The oxygen atom or
the hydrogen atoms?) oxygen
____ 18. Name the following polyatomic ions? HCO
SO
sulfite, CrO
chromate, Cr O
bicarbonate, CO
carbonate, NO
nitrite,
dichromate
____ 19. Create the proper ionic compounds with the ions in a – d. (REMEMBER THE ―CRISS CROSS‖
METHOD WE DID WITH THE ION DICE!!)
a. Ca2+, F =
c. Ba , O
=
(write the formula of the compound
(write the formula of the compound
here) ________CaF2________
here) ___BaO________
b. Na , Cl =
d. Pb , O
=
(write the formula of the compound
here) ____NaCl______
(write the formula of the compound
here) __PbO_______
____ 20. Write the correct formula for the ionic compound in a – d.
a. iron(III) sulfide Fe2O3
c. tin(II) nitride Sn3N2
b. aluminum fluoride AlF3
d. potassium bromide KBr
____ 21. Which set of chemical name and chemical formula for the same compound is correct?
a. ammonium sulfite, (NH ) S
c. lithium carbonate, LiCO
b. iron(III) phosphate, FePO
d. magnesium dichromate, MgCrO
____ 22. What is the formula for sulfurous acid? H2SO3
____ 23. List the 7 diatomic molecules? N, O, F, Cl, Br, I, H
____ 24. How many moles of copper are in 4.8
10
atoms of copper? 0.797
____ 25. How many molecules are in 2.10 mol SO ? 1.26 x 1024
____ 26. What is the molar mass of AgBr3? 347.57
____ 27. What is the volume (in liters) of one mole of a gas under STP conditions?
____ 28. What is the percent by mass of hydrogen in acetone, C H O?
22.4 L
10.4%
____ 29. What is the empirical formula of C8H24O64? CH3O8
____ 30. What is the empirical formula of a substance that is 52.2% C, 17.4% H, and 30.4% N by
weight? C2H8N
____ 31. Balance the following chemical equation?
CuCl + KOH
Cu(OH)
KCl 1:3:1:3
____ 32. In order for the reaction 2Fe
a.
b.
c.
d.
6HCl
2FeCl
3H to occur, which of the following must be true?
Fe must be above Cl on the activity series.
Fe must be above H on the activity series.
Heat must be supplied for the reaction.
A precipitate must be formed.
____ 33. Which of the following is a balanced equation representing the decomposition of tin (IV) oxide?
Sn 2O
2Sn O
a. SnO
c. Sn O
b.
SnO
Sn
O
d.
SnO
Sn
O
____ 34. A double-replacement reaction takes place when aqueous Na CO reacts with aqueous
Sn(NO ) . What are the 2 products in this reaction? NaNO3 , SnCO3
____ 35. The equation Mg(s)
2HCl(aq)
MgCl (aq)
H g is an example of which type of
reaction? Single replacement
____ 36. Balance the following equation and determine what type of reaction this is:
S(s) + O (g)  SO (g) 2:3:2 synthesis
____ 37. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of
sulfuric acid are needed to completely react with 13.2 mol of aluminum?
2Al(s) + 3H SO (aq)  Al (SO ) (aq) + 3H (g) 19.8 m
____ 38. The equation below shows the decomposition of lead (II) nitrate. How many grams of oxygen
are produced when 12.7 g NO is formed?
2.21 g
____ 39. How many liters of NH are needed to react completely with 21.4 L of NO (at STP)?
4NH (g) + 6NO(g)
5N (g) + 6H O(g)
14.27 L
____ 40. Which of the following is NOT true about limiting and excess reagents?
a. The amount of product obtained is determined by the limiting reagent.
b. A balanced equation is necessary to determine which reactant is the limiting reagent.
c. Some of the excess reagent is left over after the reaction is complete.
d. The reactant that has the smallest given mass is the limiting reagent.
____ 41. How many liters of fluorine gas can be produced when 0.98 L of HF react with excess O at
STP?
4HF(g) + O (g)
2F (g) + 2H O(g) 0.49 L
____ 42. Identify the limiting reagent and the volume of NO formed when 11 L NS reacts with 18 L O
to produce NO gas and SO gas at STP.
NS (g) + 3O (g)
NO (g) + 2SO (g) LR: oxygen ; 6 L NO2