Unit 2 Review

Chapter 4

100

a. What electron sublevel starts to fill after completion of the 3s sublevel?

b. What electron sublevel starts to fill after completion of the 3d sublevel?

a. 3p

b. 4p

200

a.  How many 3d electrons are in Fe?

b. How many 4d electrons are in I?

a. 6

b. 10

300

Of the elements Na, P, Cl, and F, which 

a. has the highest ionization energy?

b. has the largest atomic size?

c. has the highest metallic character?

a. F

b. Na

c. Na

400

Write the abbreviated electron configuration and draw the abbreviated electron orbital diagram for Cobalt.

[Ar] 4s²3d⁷

[Ar] [↑↓]   [↑↓] [↑↓] [↑ ] [↑ ] [↑ ]

4s                       3d

500

Write the unabbreviated electron configuration and draw the unabbreviated electron orbital diagram for iron.

1s²2s²2p⁶3s²3p⁶4s²3d⁶

[↑↓]  [↑↓]  [↑↓][↑↓][↑↓]  [↑↓]  [↑↓][↑↓][↑↓]  [↑↓]  [↑↓][↑][↑][↑][↑]

1s     2s          2p        3s           3p        4s           3d          

Chapter 6

100

One of the ions of tin is tin (IV).

a. What is the symbol for this ion?

b. How many protons and electrons are in the ion?

c. What is the formula of tin (IV) oxide?

d. What is the formula of tin (IV) phosphate?

a. Sn⁴⁺

b. 50 protons and 46 electrons

c. SnO₂

d. Sn₃(PO₄)₄

200

Name each of the following molecular compounds:

a. NCl₃

b. P₂O₅

c. BF₃

a. nitrogen trichloride

b. diphosphorus pentoxide

c. boron trifluoride

300

Draw the Lewis structures for the following:

H₂CCCl₂

Refer to google slides

400

Select the more polar bond in each of the following pairs:

a. C ---- N or C ---- O

b. Br ---- Cl or S ---- Cl

a. C ---- O

b. S ---- Cl

500

Classify each of the following molecules as polar or nonpolar:

a. HBr

b. NCl₃

a. polar

b. nonpolar

Chapter 6 again

100

Write the formula for each of the following ionic compounds:

a. tin (II) sulfide

b. silver chloride

c. copper (I) phosphide

a. SnS

b. AgCl

c. Cu₃P

200

Write the formula for each of the following molecular compounds:

a. carbon sulfide

b. dihydrogen sulfide

a. CS

b. H₂S

300

For each of the following, draw the lewis structures and determine the electron-group geometry and the shape:

a. NF₃

b. CSe₂

a. tetrahedral and trigonal pyramidal

b. linear and linear

Refer to google slides for lewis structures

400

Show the dipole arrow for each of the following bonds:

a. C ---- N

b. F ---- Cl

a. C ---- N

-l--->

b. F ---- Cl

<---l-

500

Indicate the major type of intermolecular forces - ionic bonds, dipole-dipole attractions, hydrogen bonds, dispersion forces - that occur between particles of the following:

Br₂

CH₃OH

dispersion forces

hydrogen bonding

Chapter 7

100

What is a chemical change?

A substance that is converted into one or more other substances with different formulas and different properties.

200

What are 2 possible observations of a chemical change?

1) formation of gas or emission of odor

2) emission of light and/or heat, or heat absorbed

3) production of a solid; from solution called a precipitate

4) color change

300

Balance each of the following chemical equations:

a. Mg(s) + AgNO₃(aq) → Mg(NO₃)₂(aq) + Ag(s)

b. Al(s) + CuSO₄(aq) → Al₂(SO₄)₃(aq) + Cu(s)

a. Mg(s) + 2 AgNO₃(aq) → Mg(NO₃)₂(aq) + 2 Ag(s)

b. 2 Al(s) + 3 CuSO₄(aq) → Al₂(SO₄)₃(aq) + 3 Cu(s)

400

How many molecules are present in 1.75 moles of carbon dioxide?

1.05 x 10²⁴ molecules of CO₂

500

Calculate the moles of Fe in 5.22 x 10²² atoms of Fe

0.0867 moles of Fe

Chapter 7 again

100

What is the molar mass of the following compound:

ZnSO₄

161.44 g/mol

200

Calculate the number of moles in the following:

25 g of CO₂

0.568 mole of CO₂

300

Balance each of the following chemical equations:

a. Pb(NO₃)₂(aq) + NaCl(aq) → PbCl₂(s) + NaNo₃(aq)

b. HCl(aq) + Al(s) → H₂(g) + AlCl₃(aq)

a. Pb(NO₃)₂(aq) + 2NaCl(aq) → PbCl₂(s) + 2NaNO₃(aq)

b. 6HCl(aq) + 2Al(s) → 3H₂(g) + 2AlCl₃(aq)

400

Calculate the mass, in grams, for the following:

1.50 moles of Na

34.5 g 

500

Calculate the number of moles for the following:

15.0 g of ammonia

0.881 mole of NH₃