Chem test II

Atomic masses are derived from calculations using experimental data. As the experiments that provide this data get more precise, the data get more accurate, and the atomic masses values reported on the periodic table are revised. One source of data from 1964 reports that the element potassium is 93.10% potassium-39, which has atoms with a mass of 38.963714 u (atomic mass units), 0.0118% potassium-40, which has atoms with a mass of 39.964008 u, and 6.88% potassium-41, which has atoms with a mass of 40.961835 u. Using this data, calculate the weighted average mass of potassium atoms, in atomic mass units. Report your answer to the fourth decimal position. The weighted average mass of potassium atoms is potassium's atomic mass. How does your calculated value compare to potassium's reported atomic mass on the periodic table in this text? (Enter the value from the table.)

(93.10*38.963714)/(100))+((6.88*40.961835)/(100))+((.0118*39.964008)/(100)) = 39.0981/1 39.10 The calculated value is slightly lower than that reported in the table

A multivitamin tablet contains 0.458 g of CaHPO4 as a source of phosphorus. The recommended daily value of phosphorus is 1.000 g of P

(b) 0.475 g CaHPO4 ✕ (1 mol CaHPO4 / 136.058 g CaHPO4) ✕ (1 mol P / 1 mol CaHPO4) ✕ (30.97 g P / 1 mol P) = 0.1081 g P ≈ 0.108 g P (c) (0.1081 g P in the supplement / 1.000 g P total recommended) ✕ 100% = 10.81% ≈ 10.8%

When atoms of the following elements form ions, what charge or charges would the ions have? ag br aluminum magnesium bromine copper sodium al

+1 -1 +3 +2 +1 -1 +1, +2 +1 +3

When atoms of the following elements form ions, what charge or charges would the ions have? magnesium Ag bromine

+2 +1 -1

(a) Magnesium ions can be precipitated from seawater as magnesium hydroxide, Mg(OH)2. Each kiloliter of seawater yields about 3.0 kg of the compound. How many metric tons of magnesium metal can be made from the magnesium hydroxide derived from 1.5 ✕ 105 kL of seawater? 1.2x105 = 1.5e+02 (b) Brucite is a natural form of magnesium hydroxide. A typical crude ore containing brucite is 26% Mg(OH)2. What minimum mass, in metric tons, of this crude ore is necessary to make 30.68 metric tons of magnesium metal? 31%, 30.55 = 2.4e+02 (HW #6)

1.5e+05 kL seawater ✕ (3.0 kg Mg(OH)2 / 1 kL seawater) ✕ (1e+03 g / 1 kg) ✕ (1 mol Mg(OH)2 / 58.326 g Mg(OH)2) ✕ (1 mol Mg / 1 mol Mg(OH)2) ✕ (24.31 g Mg / 1 mol Mg) ✕ (1 kg / 1e+03 g) ✕ (1 t / 1e+03 kg) = 188 t Mg ≈ 1.9e+02 t Mg 26% Mg(OH)2 means there are 26 g Mg(OH)2 per 100 g ore.30.68 t Mg ✕ (1e+03 kg / 1 t) ✕ (1e+03 g / 1 kg) ✕ (1 mol Mg / 24.31 g Mg) ✕ (1 mol Mg(OH)2 / 1 mol Mg) ✕ (58.326 g Mg(OH)2 / 1 mol Mg(OH)2) ✕ (100 g ore / 26 g Mg(OH)2) ✕ (1 kg / 1e+03 g) ✕ (1 t / 1e+03 kg) = 283 t ore ≈ 2.8e+02 t ore

Beryl, Be3Al2(SiO3)6, is a natural source of beryllium, a known carcinogen. What is the mass in kilograms of beryllium in 1.692 Mg of Be3Al2(SiO3)6? 1.134 = 57.04

1.692 Mg of Be3Al2(SiO3)6 ✕ (1e+06 g Be3Al2(SiO3)6 / 1 Mg Be3Al2(SiO3)6 ) ✕ (1 mol Be3Al2(SiO3)6 / 537.536 g Be3Al2(SiO3)6) ✕ (3 mol Be / 1 mol Be3Al2(SiO3)6) ✕ (9.012 g Be / mol Be) ✕ (1 kg Be/ 1e+03 g Be) = 85.101 kg Be ≈ 85.10 kg Be

A multivitamin tablet contains 11 µg of vanadium in the form of sodium metavanadate, NaVO3. How many micrograms of NaVO3 does each tablet contain?

11 µg V ✕ (1 g / 1e+06 µg) ✕ (1 mol V / 50.94 g V) ✕ (1 mol NaVO3 / 1 mol V) ✕ (121.93 g NaVO3 / 1 mol NaVO3) ✕ (1e+06 µg / 1 g) = 26.3 µg NaVO3 ≈ 26 µg NaVO3

what are the approximate bond angles between f-n:=:n-f

120 degrees

Al2O3 + C → Al + CO2 H3BO3 → B2O3 + H2O I2 + Cl2 → ICl3

2 Al2O3 + 3 C → 4 Al + 3 CO2 2 H3BO3 → B2O3 + 3 H2O I2 + 3 Cl2 → 2 ICl3

Under the right conditions, methanol reacts with oxygen to yield formaldehyde, CH2O, and water. Most of the formaldehyde made in this way is used in the production of other substances, including some important plastics. Formaldehyde, itself now a suspected carcinogen, was once used in insulation foams and in plywood adhesives. Write a balanced equation, without including states, for the reaction that produces formaldehyde from methanol.

2 CH3OH + O2 → 2 CH2O + 2 H2O

Phosphoric acid, H3PO4, is an important chemical used to make fertilizers, detergents, pharmaceuticals, and many other substances. High purity phosphoric acid is made in a two-step process called the furnace process. Ca3(PO4)2 + SiO2 + C → P4 + CO + CaSiO3 P4 + O2 + H2O → H3PO4

2 Ca3(PO4)2 + 6 SiO2 + 10 C → 6 CaSiO3 + P4 + 10 CO P4 + 5 O2 + 6 H2O → 4 H3PO4

Hydrochlorofluorocarbons (HCFCs), which contain hydrogen as well as carbon, fluorine, and chlorine, are less damaging to the ozone layer than chlorofluorocarbons (CFCs). HCFCs are therefore used instead of CFCs for many purposes. Balance the following equation that shows how the HCFC chlorodifluoromethane, CHClF2, is made. (Use the lowest possible whole number coefficients. Omit states-of-matter in your answer.)

2 HF + CHCl3 → CHClF2 + 2 HCl

2 KOH(aq) + Ni(NO3)2(aq)→

2 KOH(aq)+Ni(NO3)2(aq) → Ni(OH)2(s)+2KNO3(aq)

In the modern process for making sodium hydroxide, an electric current is run through a sodium chloride solution, forming hydrogen and chlorine along with the sodium hydroxide. Both sodium chloride and water are reactants. Write a balanced equation, without including states, for this reaction

2 NaCl + 2 H2O → 2 NaOH + Cl2 + H2

Write a conversion factor that converts between moles of nitrogen in dinitrogen pentoxide, N2O5, and moles of N2O5

2 mol n/1 mol n2o5

sb2s3(s) + o2(g) --> sb2o3(s) + so2(g)

2 sb2s3(s) + 9 o2(g) --> 2 sb2o3(s) + 6 so2(g)

Pig iron is iron with about 4.3% carbon in it. The carbon lowers the metal's melting point and makes it easier to shape. To produce pig iron, iron(III) oxide is combined with carbon and oxygen at high temperature. Three changes then take place to form molten iron with carbon dispersed in it. Write a balanced equation, without including states, for each of these changes. (a) Carbon combines with oxygen to form carbon monoxide (b) Iron(III) oxide combines with the carbon monoxide to form iron and carbon dioxide (c) Carbon monoxide changes into carbon (in the molten iron) and carbon dioxide

2C + O2 → 2 CO Fe2O3 + 3 CO → 2 Fe + 3 CO2 2 CO → C+CO2

3 Cd(NO3)2(aq) + 2 K3PO4(aq)→

3 Cd(NO3)2(aq) + 2 K3PO4(aq) → Cd3(PO4)2(s) + 6 KNO3(aq)

Chlorofluorocarbons (CFCs) are compounds that contain carbon, fluorine, and chlorine. Because they destroy ozone that forms a protective shield high in earth's atmosphere, their use is being phased out, but at one time they were widely employed as aerosol propellants and as refrigerants. Balance the following equation that shows how the CFCs dichlorodifluoromethane, CCl2F2, and trichlorofluoromethane, CCl3F, are produced.

3 HF + 2 CCl4 → CCl2F2 + CCl3F + 3 HCl

For each of the following pairs of compounds, write the complete equation for the neutralization reaction that takes place when the substances are mixed. a) Al(OH)3(s) + HNO3(aq) b) H2SO3(aq) + LiOH(aq) c) KHCO3(aq) + HF(aq)

3 HNO3(aq) + Al(OH)3(s) → Al(NO3)3(aq) + 3 H2O(l) H2SO3(aq) + 2 LiOH(aq) → Li2SO3(aq) + 2 H2O(l) HF(aq) + KHCO3(aq) → KF(aq) + H2O(l) + CO2(g)

For each of the following pairs of formulas, predict whether the substances they represent would react to yield a precipitate. KOH(aq) + Cr(NO3)3(aq) NaBr(aq) + AgNO3(aq) Fe(NO3)3(aq) + K3PO4(aq)

3 KOH(aq) + Cr(NO3)3(aq) → 3 KNO3(aq) + Cr(OH)3(s) NaBr(aq) + AgNO3(aq) → NaNO3(aq) + AgBr(s) Fe(NO3)3(aq) + K3PO4(aq) → FePO4(s) + 3 KNO3(aq)

Manganese(II) phosphate is used to coat steel, aluminum, and other metals to prevent corrosion. It is produced in the reaction between solid manganese(II) hydroxide and aqueous phosphoric acid. Write the complete equation for this reaction

3 Mn(OH)2(s) + 2 H3PO4(aq) → Mn3(PO4)2(s) + 6 H2O(l)

When the explosive liquid nitroglycerin, C3H5N3O9, decomposes, it forms carbon dioxide gas, nitrogen gas, water vapor, and oxygen gas. Write a complete, balanced equation for this reaction

4 C3H5N3O9(l) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)

Nitric acid, HNO3, which is used to make fertilizers and explosives, is made industrially in the three steps described below. Write a balanced equation, without including states, for each of these steps. (a) Ammonia reacts with oxygen to form nitrogen monoxide and water. (b) Nitrogen monoxide reacts with oxygen to form nitrogen dioxide. (c) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide.

4 NH3 + 5 O2 → 4 NO + 6 H2O 2 NO + O2 → 2 NO2 3 NO2 + H2O → 2 HNO3 + NO

cl(g) + ch4(g) + o2(g) --> hcl(g) + co(g)

4 cl2(g) + 2 ch4(g) --> 8 hcl(g) + 2 co(g)`

As a member of the corundum family of minerals, sapphire (the September birthstone) consists primarily of aluminum oxide, Al2O3. Small amounts of iron and titanium give it its rich dark blue color. Gem cutter Norman Maness carved a giant sapphire into the likeness of Abraham Lincoln. If this 2302-carat sapphire were pure aluminum oxide, how many moles of Al2O3 would it contain? (There are exactly 5 carats per gram.)

4.514 or 4.515

Thortveitite is a natural ore that contains from 37% to 42% scandium oxide, Sc2O3. Scandium metal is made by first reacting the Sc2O3 with ammonium hydrogen fluoride, NH4HF2, to form scandium fluoride, ScF3. The scandium in ScF3 is reduced to metallic scandium in a reaction with calcium. What is the maximum mass, in kilograms, of scandium metal that can be made from 1420.0 kilograms of thortveitite that is 42% Sc2O3?

42% Sc2O3 means there are 42 g Sc2O3 per 100 g ore.1420.0 kg ore ✕ (1e+03 g / 1 kg) ✕ (42 g Sc2O3 / 100 g ore) ✕ (1 mol Sc2O3 / 137.92 g Sc2O3) ✕ (2 mol Sc / 1 mol Sc2O3) ✕ (44.96 g Sc / 1 mol Sc) ✕ (1 kg / 1e+03 g) = 389 kg Sc ≈ 3.9e+02 kg Sc

Some forms of hematite, a mineral composed of iron(III) oxide, can be used to make jewelry. Because of its iron content, hematite jewelry has a unique problem among stone jewelry. It shows signs of rusting. How many moles of iron are there in a necklace that contains 71.429 g of Fe2O3

71.429 g Fe2O3 ✕ (1 mol Fe2O3 / 159.7 g Fe2O3) ✕ (2 mol Fe / 1 mol Fe2O3) = 0.89454 mol Fe ≈ 8.945e−01 mol Fe

An extremely explosive ionic compound is made from the reaction of silver compounds with ammonia. A sample of this compound is found to contain 15.785 g of silver and 0.683 g of nitrogen. 15.556 silver, .673 nitrogen Ag3N

Ag = 15.785g*1mol/107.87g = .1463 N = .683g*1mol/14.01=.04889 Ag = .1463/.04889 N = .04889/.04889 Ag3N

The taste of drinking water can be improved by removing impurities from our municipal water by adding substances to the water that precipitate a solid (called a flocculent) that drags down impurities as it settles. One way this is done is to dissolve aluminum sulfate and sodium hydroxide in the water to precipitate aluminum hydroxide. Write the complete equation for this reaction

Al2(SO4)3(aq)+ 6 NaOH(aq) → 2 Al(OH)3(s)+ 3 Na2SO4(aq)

Aluminum sulfate, commonly called alum, is used to coat paper made from wood pulp

Al2O3 + 3 H2SO4 → Al2(SO4)3 + 3 H2O

Phosphate ions find their way into our water system from the fertilizers dissolved in the runoff from agricultural fields and from detergents that we send down our drains. Some of these phosphate ions can be removed by adding aluminum sulfate to the water and precipitating the phosphate ions as aluminum phosphate. Write the net ionic equation for the reaction that forms the aluminum phosphate.

Al^3+(aq) + PO4^3-(aq) → AlPO4(s)

Type the formula that corresponds to the name gold(III) sulfate.

Au2(SO4)3

B2O3(s) + NaOH(aq) → Na3BO3(aq) + H2O(l) Al(s) + H3PO4(aq) → AlPO4(s) + H2(g) C6H14(l) + O2(g) → CO2(g) + H2O(l)

B2O3(s)+6 NaOH(aq) → 2 Na3BO3(aq)+3 H2O(l) 2Al(s)+2H3PO4(aq) → 2AlPO4(s)+3H2(g) 2C6H14(l)+19O2(g) → 12CO2(g)+14H2O(l)

Type the formula for barium acetate.

Ba(C2H3O2)2

Write the chemical formula that corresponds to the name tribromine octoxide

Br3O8

Ca3(PO4)2 + H2SO4 → H3PO4 + CaSO4

Ca3(PO4)2 + 3 H2SO4 → 2 H3PO4 + 3 CaSO4

CaCN2 + H2O → CaCO3 + NH3 HClO4 + Fe(OH)2 → Fe(ClO4)2 + H2O NaClO3 → NaCl + O2

CaCN2 + 3 H2O → CaCO3 + 2NH3 2 HClO4 + Fe(OH)2 → Fe(ClO4)2 + 2 H2O 2 NaClO3 → 2 NaCl + 3 O2

CaCO3(s) + 2 HNO3(aq) → Ca(NO3)2(aq)+ H2O(l) +_____

CaCO3(s) + 2 HNO3(aq) → Ca(NO3)2(aq)+ H2O(l) + CO2(g)

Industrial chemists make hydrofluoric acid (which is used in aluminum and uranium processing, to etch glass, and to make CFCs) from the reactions of aqueous calcium fluoride and aqueous sulfuric acid. Write the complete equation for this reaction.

CaF2(aq) + H2SO4(aq) → CaSO4(s) + 2 HF(aq)

Write a complete, balanced chemical equation for the reaction between water solutions of iron(III) chloride and silver nitrate. (Use the lowest possible whole number coefficients.

FeCl3 (aq) + 3 AgNO3(aq) → Fe(NO3)3(aq) + 3 AgCl(s)

One of the substances used to make nylon is hexanedioic acid, HO2CCH2CH2CH2CH2CO2H. This diprotic weak acid is also called adipic acid. Write the equation for the complete reaction between this acid and sodium hydroxide. (The acidic hydrogen atoms are on each end of the formula. Use the lowest possible coefficients.

H2C6H8O4(aq) + 2 NaOH(aq) → 2 H2O(l) + Na2C6H8O4(aq)

Which of the following are found in a solution of the strong acid hydrochloric acid?

H3O+ and Cl−

Which of the following are found in a solution of the weak acid acetic acid?

H3O+, C2H3O2−, and larger amounts of HC2H3O2

write the complete equation for the neutralization reaction that takes place when the substances are mixed HBr(aq) + NaOH(aq)

HBr(aq) + NaOH(aq) --> NaBr(aq) + H2O(l)

Type the formula for the conjugate acid of F−

HF

Type the formula for nitric acid.

HNO3

HNO3(aq) + NaHCO3(aq) → _____ + CO2(g) + NaNO3(aq)

HNO3(aq) + NaHCO3(aq) → H2O(l) + CO2(g) + NaNO3(aq)

Type the formula for the conjugate acid of SO32-

HSO3-

Write the chemical formula that corresponds to the name iodine tribromide

IBr3

At the instant that water solutions of KOH and HCl are mixed, the following particles are found in solution.

K+ ions, OH− ions, H3O+ ions, Cl− ions, and H2O molecules

KOH(aq) + HCl(aq)→ _____ + H2O(l)

KOH(aq) + HCl(aq) → KCl(aq) + H2O(l)

Write the complete equation for the neutralization reactions that take place when the following water solutions are mixed (a) KOH(aq) + HF(aq) (b) H2SO4(aq) + NaOH(aq) (c) HCl(aq) + LiOH(aq)

KOH(aq) + HF(aq) → H2O(l) + KF(aq) H2SO4(aq) + 2 NaOH(aq) → Na2SO4(aq) + 2 H2O(l) HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)

Write the complete equation for the neutralization reactions that take place when the following water solutions are mixed. (a) LiOH(aq) + HNO2(aq) (b) Co(OH)2(s) + HNO3(aq) (c) H3PO4(aq) + KOH(aq)

LiOH(aq) + HNO2(aq) → H2O(l) + LiNO2(aq) Co(OH)2(s) + 2 HNO3(aq) → Co(NO3)2(aq) + 2 H2O(l) H3PO4(aq) + 3 KOH(aq) → 3 H2O(l) + K3PO4(aq)

Type the formula that corresponds to the name manganese(II) phosphide

Mn3P2

An ionic compound that is 22.071% manganese, 1.620% hydrogen, 24.887% phosphorus, and 51.422% oxygen is used as a food additive and dietary supplement.

MnH4P2O8

Identify the Brønsted-Lowry base for the forward reaction below. NH3(aq) + HNO2(aq)NH4+(aq) + NO2−(aq)

NH3

Type the formula for the conjugate base of NH4+

NH3

All of the equations for the production of nitric acid can be summarized in a single equation, called a net equation, that describes the overall change for the complete process. This equation shows ammonia combining with oxygen to yield nitric acid and water. Write a balanced equation, without including states, for this net reaction

NH3 + 2 O2 → HNO3 + H2O

A solution of ammonia, NH3, contains

NH4+ ions, OH− ions, and larger amounts of NH3 molecules.

For each of the following pairs of formulas, predict whether the substances they represent would react to yield a precipitate a) NaCl(aq) + Al(NO3)3(aq) b) MnCl2(aq) + Na3PO4(aq) c) Zn(C2H3O2)2(aq) + Na2CO3(aq)

NONE 3 MnCl2(aq) + 2 Na3PO4(aq) → 6 NaCl(aq) + Mn3(PO4)2(s) Zn(C2H3O2)2(aq) + Na2CO3(aq) → ZnCO3(s) + 2 NaC2H3O2(aq)

A solution of sodium carbonate, Na2CO3, contains

Na+ ions, OH− ions, CO32-, and HCO3− ions.

Sodium tripolyphosphate, Na5P3O10, is called a "builder" when added to detergents. It helps to create the conditions in laundry water necessary for the detergents to work most efficiently. When phosphoric acid, H3PO4, is combined with sodium carbonate, three reactions take place in the mixture that lead to the production of sodium tripolyphosphate. (a) Phosphoric acid reacts with sodium carbonate to form sodium dihydrogen phosphate, water, and carbon dioxide (b) Phosphoric acid also reacts with sodium carbonate to form sodium hydrogen phosphate, water, and carbon dioxide (c) Sodium dihydrogen phosphate combines with sodium hydrogen phosphate to yield sodium tripolyphosphate and water

Na2CO3 + 2 H3PO4 → H2O + CO2 + 2 NaH2PO4 Na2CO3 + H3PO4 → Na2HPO4 + CO2 + H2O NaH2PO4 + 2 Na2HPO4 → Na5P3O10 + 2 H2O

Sodium hydroxide, which is often called caustic soda, is used to make paper, soaps, and detergents. For many years, it was made from the reaction of sodium carbonate with calcium hydroxide (also called slaked lime). The products are sodium hydroxide and calcium carbonate. Write a balanced equation, without including states, for this reaction

Na2CO3 + Ca(OH)2 → 2 NaOH + CaCO3

Write the complete equation for the following precipitation reaction 2 NaBr(aq) + Pb(NO3)2(aq)→

Pb(NO3)2(aq) + 2 NaBr(aq) → 2 NaNO3(aq) + PbBr2(s)

Write the chemical formula that corresponds to the name phosphorus pentachloride

Pcl5

Type the formula for the conjugate base of HSO3-

SO2-3

type the formula for the zinc ion

Zn2+

Butanoic acid, CH3CH2CH2CO2H, is a monoprotic weak acid that is responsible for the smell of rancid butter. (a) Write the formula for the conjugate base of this acid. (b) Write the equation for the reaction between this acid and water, and indicate the Brønsted-Lowry acid and base for the forward Brønsted-Lowry acid Brønsted-Lowry base

a) CH3CH2CH2CO2- b)CH3CH2CH2CO2H + H2O → CH3CH2CH2CO2- + H3O+ CH3CH2CH2CO2H H2O

Covalent bonds usually form in order to

both pair unpaired electrons and allow atoms to gain an octet of valence electrons around them.

In 1989 a controversy arose concerning the chemical daminozide, or Alar®, which was sprayed on apple trees to yield redder, firmer, and more shapely apples. Concerns about Alar's safety stemmed from the suspicion that one of its breakdown products, unsymmetrical dimethylhydrazine (UDMH), was carcinogenic. Alar is no longer sold for food uses. UDMH has the empirical formula of CNH4 and has a molecular mass of 60.099

c2n2h8

Because particles with opposite charges attract each other, there is an attraction between _ and _ This attraction is called an ionic bond.

cations, anions

a(n) _ is a concise written description of the components of a chemical compound

chemical formula

Type the name of the Cl− ion. Do not type "ion" as part of the name.

chloride

Type the formula that corresponds to the name chromium(III) bromide.

crbr3

for each of the lewis structures given below Br-b-i-br

electron group - trigonal planar, 120, trigonal planar

The geometry that describes all of the electron groups around an atom in a molecule is called its electron group geometry

electron groups

Of the three ways used to represent molecules (space-filling model, ball-and-stick model, and geometric sketch), the geometric sketch shows a simple way to represent a three-dimensional structure with a two-dimensional drawing.

geometric sketch

Type the formula that corresponds to the name potassium oxide.

k_2O

what is the electron group geometry around the carbon atom in the following molecule? o=c=o

linear

Paired valence electrons are called

lone pairs

Metallic atoms hold some of their electrons relatively loosely, and as a result, they tend to _ electrons and form cations. In contrast, nonmetallic atoms attract electrons more strongly than metallic atoms, so nonmetals tend to _ electrons and form anions.

lose, gain true

A defoliant is an herbicide that removes leaves from trees and growing plants. One ionic compound used for this purpose is 12.711% magnesium, 37.083% chlorine, and 50.206% oxygen.

mgcl2o6

Compounds that are composed of collections of atoms held together by all covalent bonds are called _ compounds

molecular

How many valence electrons do the atoms of each of the following elements have? Write the electron configuration for these electrons number of valence electrons? neon, ne boron, b oxygen, o phosphorus, p

neon 8 2s^2 2p^6 boron 3 2s^22p^1 oxygen 6 2s^2 2p^4 phosphorus 5 3s2 3 p3

When the difference in electron-attracting ability for the atoms in a bond is negligible (or zero), the bond is called a(n)

nonpolar covalent

The cations in solutions of ionic compounds are surrounded by the

oxygen ends of water molecules, which have a partial negative charge.

An ionic compound that is 62.56% lead, 8.46% nitrogen, and 28.98% oxygen is used as a mordant in the dyeing industry. A mordant helps to bind a dye to the fabric.

pbn2o6 lead(II) nitrate

a(n) _ is a charged collection of atoms held together by covalent bonds

polyatomic ions

what's wrong with the following Lewis Structure

the sulfur atom and one of the chlorine atoms do not have their most common bonding pattern

which of the following statements best describes the following structure

they represent different substances that are no isomers

what is the molecular geometry around the arsenic atom i-as-i-i-:

trigonal pyramid

Although silver can form +1 and +2 cations, the +2 is so rare that we usually name Ag+ silver ion, not silver(I) ion. Ag2+ is named silver(II) ion

true

Mixtures are samples of matter that contain two or more pure substances and have _ composition

variable

strong acid hydrochloric acid, hcl water insoluble chromium(III) hydroxide, cr(oh)3 the instant the two solutions are mixed the solutions contain the following

water molecules, hydroxide ions, chromium ions, hydronium ions, chloride ions