Honors Chem Unit 4 Review

HONORS CHEM UNIT 4 REVIEW

UNIT 4 TOPICS

Ch. 5 Nomenclature

-Naming ionic, molecular, and acid compounds from their formulas

-Writing chemical formulas from the names of ionic, molecular, and acid compounds

Ch. 12 Chemical Bonding

-What is a chemical bond?

-What are the three types of chemical bonding that we have talked about?

-What are the characteristics of each of these bonds?

-Writing electron configurations for ions

-Electronegativity.

-Determining whether or not a bond is polar or not

-Drawing Lewis structures

-Using VSEPR theory to predict molecular shapes

-Determining molecular polarity

Complete the following chart:

H2CrO4
magnesium chloride
AgCl
KNO3
diphospohorus pentoxide
Ba(ClO3)
KMnO4
tin(IV) chloride
SO3
aluminum hydroxide
Cu(NO3)2
KClO
PbO2
nitrous acid
NaClO4
H2C2O4
silicon dioxide
potassium cyanide
potassium perchlorate
Ag3PO4
NO3
CO
FeO
lead(II) chromate
barium nitride

1. The electron pair in a bond could be considered

[A] closer to C because carbon has a lower electronegativity than fluorine

[B] an inadequate model because the bond is ionic

[C] centrally located directly between the C and F

[D] closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair

[E] closer to F because fluorine has a higher electronegativity than carbon

2. What is the correct order of the following bonds in terms of decreasing polarity?

[A] [B] [C]

[D] [E]

3. Which of the following bonds would be the most polar without being considered ionic?

[A] [B] [C] [D] [E]

4. Use the following choices to classify the bonds in each of the following molecules.

a. nonpolar

b. polar

I2 ______

5. Which of the following elements has the lowest electronegativity?

[A] Cl [B] S [C] Rb [D] Ca [E] Na

6. Which of the following has nonpolar bonds?

[A] H2S [B] OF2 [C] Br2 [D] HCl [E] All are nonpolar.

7. Which of the following is the most electronegative?

[A] Mg [B] Cl [C] Na [D] P [E] Si

8. The F- and O2- ions have the same electron configuration.

[A] True [B] False

9. Which element or ion listed below has the electron configuration 1s22s22p63s23p6?

[A] Cl [B] Ca2+ [C] Se [D] Br- [E] two of these

11. Which of the following species would be expected to have the lowest ionization energy?

[A] Br- [B] Se2- [C] Rb+ [D] Kr [E] Sr2+

12. Which of the following has the smallest radius?

[A] Ar [B] Ca2+ [C] Cl- [D] S2- [E] K+

13. Which of the following ions has the same electron configuration as an argon atom?

[A] S3- [B] P3+ [C] Br- [D] K+ [E] Ca+

14. 1s22s22p63s23p6 is the electron configuration for which one of the following ions?

[A] F- [B] S2- [C] Ca+ [D] Na+ [E] none of these

15. Magnesium reacts with sulfur to form

[A] MgS2 [B] MgS [C] Mg2S [D] Mg2S3 [E] none of these

16. Write the electron configuration for Sr2+.

17. How many lone pairs of electrons are in the Lewis structure for ammonia, NH3?

[A] 2 [B] 4 [C] 1 [D] 0 [E] 3

18. The Lewis structure for which of the following contains the greatest number of lone pairs of electrons?

[A] CH4 [B] F2 [C] HF [D] H2 [E] H2O

19. Choose the correct Lewis structure for the NH4+ ion.

[A] [B] [C]

[D]

[E] none of these

20. Draw the Lewis electron structure for the AsH3 molecule.

21. Draw the Lewis structure for NI3.

22. Draw the Lewis structure for CO32-.

23. How many resonance structures are there for SO3?

24. Draw the Lewis structure for HCCl3.

25. Select the correct molecular structure for CO2 from the choices below.

a. linear

b. bent

c. pyramidal

d. tetrahedral

e. none of these