Final Review

Front 1

Unit 5

Back 1

ch 3

Front 2

Which of the following is a molecular element?

Back 2

I

Front 3

Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

Back 3

C3H6O

Front 4

Determine the name for TiCO3. Remember that titanium forms several ions.

Back 4

titanium (II) carbonate

Front 5

What is the charge on the Cr ions in Cr2O3?

Back 5

3+

Front 6

Give the correct formula for aluminum sulfate.

Back 6

Al2(SO4)3

Front 7

Give the formula for sulfurous acid.

Back 7

H2SO3

Front 8

Give the name for PBr3.

Back 8

phosphorus tribromide

Front 9

Calculate the molar mass of H2CO3.

Back 9

62.03 g/mol

Front 10

Calculate the mass percent composition of sulfur in Al2(SO4)3.

Back 10

21.38 %

Front 11

How many atoms of carbon are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.

Back 11

3.68 × 1023 C atoms

Front 12

How many molecules of butane are contained in 25.0 mL of butane? The density of butane is 0.6011 g/mL and the molar mass is 58.12 g/mol.

Back 12

1.56 × 1023 molecules butane

Front 13

Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl.

Back 13

PCl3

Front 14

Give a possible molecular formula for C3H5ClO

Back 14

C6H10Cl2O2

Front 15

What is the chemical formula for iron(III) sulfate?

Back 15

Fe2(SO4)3

Front 16

The chemical formula for the sulfite ion is

Back 16

S 2-

Front 17

How many moles are there in 3.00 g of ethanol, CH3CH2OH?

Back 17

0.0652 mol

Front 18

Which of the following has the greatest mass?

Back 18

3.88 × 1022 molecules of O2

Front 19

Which one of the following is not an empirical formula?

Back 19

C2H4O2

Front 20

Which of the following elements has the least tendency to form an ion?

Back 20

Kr

Front 21

Which of the following is an ionic compound?

Back 21

Mg3(PO4)2

Front 22

Unit 6

Back 22

ch 9

Front 23

How many lone pairs of electrons are on the As atom in AsCl3?

Back 23

1

Front 24

In the best Lewis structure for NO +, what is the formal charge on the N atom?

Back 24

0

Front 25

Which of the following processes are endothermic?

Back 25

the reaction associated with the ionization energy of potassium.

Front 26

Use the bond energies provided to estimate ΔH°rxn for the reaction below.

C2H4(g) + H2(g) → C2H6(g) ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
C-C 347
C-H 414
C=C 611
C≡C 837
H-H 436

Back 26

-128 kJ

Front 27

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

Back 27

Al2O3

Front 28

Which of the following reactions is associated with the lattice energy of CaS (ΔH°latt)?

Back 28

Ca2(g) + S2(g) → CaS(s)

Front 29

Place the following in order of decreasing magnitude of lattice energy.

NaF RbBr KCl

Back 29

NaF > KCl > RbBr

Front 30

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Back 30

AlN

Front 31

Give the complete electronic configuration for S2-.

Back 31

1s22s22p63s23p6

Front 32

Identify the compound with metallic bonding.

Back 32

Li

Front 33

Identify the shortest bond.

Back 33

triple covalent bond

Front 34

Place the following elements in order of increasing electronegativity.

Sr N Na

Back 34

Sr < Na < N

Front 35

Which molecule or compound below contains a pure covalent bond?

Back 35

Cl2

Front 36

Choose the best Lewis structure for BeF2.

Back 36

Front 37

Give the number of valence electrons for ICl5.

Back 37

42

Front 38

Choose the best Lewis structure for SO42.

Back 38

Front 39

Draw the Lewis structure for CO32- including any valid resonance structures. Which of the following statements is TRUE?

Back 39

The CO32- ion contains two C-O single bonds and one C=O double bond.

Front 40

Draw the best Lewis structure for the free radical, NO2. What is the formal charge on the N?

Back 40

+1

Front 41

Which compound has the highest carbon-carbon bond strength?

Back 41

HCCH

Front 42

Place the following in order of increasing bond length.

NO2 NO3 NO

Back 42

NO < NO2 < NO3

Front 43

Unit 7

Back 43

ch 10

Front 44

Give the approximate bond angle for a molecule with a trigonal planar shape.

Back 44

120°

Front 45

Using the VSEPR model, the molecular geometry of the central atom in BF3 is __________.

Back 45

trigonal planar

Front 46

Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.

Back 46

C1 = trigonal planar, C2 = tetrahedral

Front 47

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule.

N2O NCl3 NO2

Back 47

N2O > NO2 > NCl3

Front 48

How many of the following molecules are polar?

BrCl3 CS2 SiF4 SO3

Back 48

1

Front 49

Choose the compound below that contains at least one polar covalent bond, but is nonpolar.

Back 49

CF4

Front 50

Identify the number of electron groups around a molecule with sp2 hybridization.

Back 50

3

Front 51

A molecule containing a central atom with sp3d hybridization has a(n) __________ electron geometry.

Back 51

trigonal bipyramidal

Front 52

Draw the Lewis structure for H3O+. What is the hybridization on the O atom?

Back 52

sp3

Front 53

Draw the Lewis structure for BrF5. What is the hybridization on the Br atom?

Back 53

sp3d2

Front 54

How many of the following molecules have sp3d hybridization on the central atom?

SiCl4 BrF5 AsF5 BrF3

Back 54

2

Front 55

List the number of sigma bonds and pi bonds in a single bond.

Back 55

1 sigma, 0 pi

Front 56

Draw the Lewis structure for the molecule C3H4. How many sigma and pi bonds does it contain?

Back 56

6 sigma, 2 pi

Front 57

Use the molecular orbital diagram shown to determine which of the following is most stable.

Back 57

O22

Front 58

Draw the molecular orbital diagram shown to determine which of the following is most stable.

Back 58

C22

Front 59

Using the VSEPR model, the molecular geometry of the central atom in NCl3 is __________.

Back 59

trigonal pyramidal

Front 60

What are the F-Po-F bond angles in PoF6 ?

Back 60

90°

Front 61

The hybrid orbital set used by the central atom in KrF2 is __________.

Back 61

sp3d

Front 62

Using the VSEPR model, the electron-domain geometry of the central atom in BrF4- is __________.

Back 62

octahedral

Front 63

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2.

Back 63

eg=trigonal bipyramidal, mg=linear

Front 64

Unit 8

Back 64

ch 4

Front 65

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced?

Back 65

78.4 g

Front 66

How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3?
Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s)

Back 66

48.5 mL

Front 67

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol.

BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)

Back 67

56.0g HCl

Front 68

Which of the following solutions will have the highest concentration of chloride ions?

Back 68

0.10 M AlCl3

Front 69

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL.

Back 69

0.0313 M

Front 70

Identify HCl.

Back 70

strong electrolyte, strong acid

Front 71

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed.

Back 71

H22+(aq) + OH-(aq) → H2(OH)2(l)

Front 72

What element is undergoing oxidation (if any) in the following reaction?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

Back 72

C

Front 73

How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

Back 73

2.75

Front 74

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed?
AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq)

Back 74

1.07 g

Front 75

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the chemical equation:
2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq).

Back 75

24.9 mL

Front 76

The mixing of which pair of reactants will result in a precipitation reaction?

Back 76

0.747

Front 77

What is the oxidation number of the oxygen atom in Na2O2 ?

Back 77

-1

Front 78

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?

2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)

Back 78

86.1 mL

Front 79

Which of the following pairs of aqueous solutions will form a precipitate when mixed?

Back 79

Hg2(NO3)2 + LiI

Front 80

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)?

Back 80

0.114 M

Front 81

What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Back 81

2.28

Front 82

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?

Back 82

1.02 M

Front 83

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3.

2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl

Back 83

2.78 × 1024 molecules HCl