Chemistry Chapter 3

CoCl2 * 6H2O

cobalt (II) chloride hexahydrate

CO(NO3)2 * 2H2O

cobalt (II) nitrate dihydrate

Co2(SO4)3

cobalt (III) sulfate

HIO3 (aq)

iodic acid

NiBr2 * 3H20

nickel (II) bromide trihydrate

NiCO3

nickel (II) carbonate

NiSO4 * 7H2O

nickel (II) sulfate heptahydrate

HNO3

nitric acid

NO2

nitrogen dioxide

NH3

nitrogen trihydride

NI3

nitrogen triiodide

OF2

oxygen difluoride

PCl5

phosphorus pentachloride

KHSO3

potassium hydrogen sulfite

Co(NO3)2

Cobalt (II) Nitrate

CuCO3

Copper (II) Carbonate

CuF2

Copper (II) fluoride

Li2CO3

Lithium Carbonate

CrBr2

Chromium (II) Bromide

(NH4)3PO4

ammonium phosphate

(NH4)2SO4

ammonium sulfate

Cr2S3

chromium (III) sulfide

N2O5

dinitrogen pentoxide

Na2CO3 * 10H20

sodium carbonate decahydrate

NaNO2

sodium nitrite

Na2SO4 * 7H2O

sodium sulfate heptahydrate

Copper

A certain metal hydroxide, M(OH)2, contains 32.8% oxygen by mass. What is the identity of the metal M?

6.66 mol of Carbon, 19.8 Hydrogen mol

A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound. How many moles of each element are in this sample?

80.0% Carbon, 20.0% Hydrogen

A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound. How many grams of each element are in this sample?

1.51×1023 molecules

A flask contains 0.250 mol of liquid bromine, Br2. Determine the number of bromine molecules present in the flask.

The molecular weight of C9H20 is 9*12 + 20*1 = 128 (grams/mole) and the carbon is 108/128 of that = 84.375% carbon and 15.625% hydrogen (84.28% Carbon , 15.72% Hydrogen) = 100%

A hydrocarbon is a compound that contains mostly carbon and hydrogen. Calculate the percent composition (by mass) of the following hydrocarbon: C9H20

AlCl3

Aluminum Chloride

NH4I

Ammonium Iodide

C4H6Ba04

Barium Acetate

Ionic usually have high melting points: 1)The solid in Bottle A: melts at 801 ∘C 3)The solid in bottle C melts at 825 ∘C Molecular usually have low melting points: 2)The solid in bottle B melts at 150 ∘C.

Based on the melting points, classify each compound as ionic or molecular. 1)The solid in Bottle A: melts at 801 ∘C 2)The solid in bottle B melts at 150 ∘C. 3)The solid in bottle C melts at 825 ∘C

CH3

Based on the mole ratio you determined in Part C, what is the empirical formula of this compound?

CaO3P

Calcium Phosphite

1.00 x10^24/6.02x10^23 = 1.661 moles 1 mol of H2O weighs 18g 1.661 * 18 = 29.9 g

Calculate the mass of 1.00×1024 (a septillion) molecules of water.

BeO

Enter the formula for the compound beryllium oxide.

Co3(PO4)2

Enter the formula for the compound cobalt(II) phosphate

5.563g CO2 * 1 molCO2 / 44.01g CO2 to get the amt of moles in CO2 .1264 mol CO2 * 1 mol C / 1 mol CO2 gets amt of C moles in 1 CO2 mol .1264 mol C 1.627 g H20 1.627 g H20 * 1 mol H20 / 18.016 g H2O gets amt of moles in H2O .0903 mol H2O* 2 mol H/1 mol H2O gets amt of H moles in 1 H20 mol .1806 mol H Now in order to find the oxygen you have to .1264 mol C * 12.01 g C/ 1 mol C = 1.518 g C .1806 mol H * 1.008 g H/ 1 mol H = .1820 g H Now subtract these values from the sample 1.893g - (1.518 g C + .1820 g H) = .193 Then Mol O = .193 g O * 1 mol O/ 16.00 g O = .0121 mol O Now divide all of the moles of C,H, and O by lowest value .1264 mol C/ .0121 mol O = 10.45 = 10.5 .1806 mol H/ .0121 mol O = 14.96 = 15 .0121 mol O/ .0121 mol O = 1= 1 so now you must get whole numbers so, you need 10.5 to be whole so, 10.5 *2 =21, now multiply everything by 2 the answer is C21H30O2

Find the molecular formula for progesterone.

Iron (III) Sulfate

Give the systematic name for the compound Fe2(SO4)3.

Magnesium Nitrate

Give the systematic name for the compound Mg(NO3)2

FePO4

Iron (III) Phosphate

Pb(CIO2)2

Lead (II) Chlorite

MgSO4

Magnesium Sulfate

magnesium sulfate heptahydrate

Name the hydrate MgSO4⋅7H2O.

Ni(BrO4)2

Nickel (II) Perbromate

NaBr

Sodium Bromide

Na2SO4

Sodium Sulfate

NaIO3

Sodium iodate

Sr(OH)2

Strontium Hydroxide

4.00g C4H10 x (1 mol C4H10)/(58.12g C4H10) = 0.068823 mol C4H10 second: convert moles to molecules(using avogadros number) 0.068823 mol C4H10 x (6.022x10^23 molecules C4H10)/(1 mol C4H10) = 4.14452x10^22 molecules C4H10 third: there are 4 carbon atoms in 1 molecule of butane, so use the following ratio: 4.14452x10^22 molecules C4H10 x (4 atoms C)/(1 molecule C4H10) = 1.66x10^23 atoms C (3 significant figures)

The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 4.00 g of butane?

P2O3

What is the empirical formula for the compound P4O6?

HClO2

What is the formula for chlorous acid?

H2SO3

What is the formula for sulfurous acid?

diboron hexahydride

What is the name for the compound B2H6?

phosphorus pentachloride

What is the name for the compound PCl5?

carbonic acid

What is the name of the acid whose formula is H2CO3?

Hydroiodic Acid

What is the name of the acid whose formula is HI?

ZnCl2

Zinc Chloride

BaBr2

barium bromide

BaCl2 * 2H2O

barium chloride dihydrate

Ba(OH)2 * H2O

barium hydroxide octahydrate

HBrO3 (aq)

bromic acid

CS2

carbon disulfide

H2CO3

carbonic acid

HCIO3

chloric acid

HClO2

chlorous acid

CuSO4 * 5H2O

copper (II) sulfate pentahydrate

B2Cl2

diboron dichloride

HCN (aq)

hydrocyanic acid

HF (aq)

hydrofluoric acid

HCI

hydrogen chloride

HF

hydrogen fluoride

HI (aq)

hydroiodic acid

HBrO (aq)

hypobromous acid

HCIO

hypochlorous acid

Fe(NO3)3 * 6H2O

iron (II) nitrate hexahydrate

FeSO3

iron (II) sulfite

FeCl3 * 2H2O

iron (III) chloride dihydrate

Fe2O3

iron (III) oxide

MgSO4 * 7H20

magnesium sulfate heptahydrate

Hg2SO4

mercury(I) sulfate

SiC

silicon carbide

SiO2

silicon dioxide

SiF4

silicon tetrafluoride

AgCn

silver cyanide

SF6

sulfur hexafluoride

SO3

sulfur trioxide

H2SO4 (aq)

sulfuric acid

H2SO3

sulfurous acid

P4O10

tetraphosphorus decoxide

P4S3

tetraphosphorus trisulfide

TiO2

titanium (IV) oxide