Chapter 3 – Chemistry – Flashcards

An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between 2 nonmetal atoms.
E) the attraction between 2 metal atoms.

A covalent bond is best described as
A) the sharing of electrons between atoms.
B) the transfer of electrons.
C) a bond between a metal and a nonmetal.
D) a bond between a metal and a polyatomic ion.
E) a bond between two polyatomic ions.

What is the empirical formula for C4H10O2?
A) C2H5O
B) CHO
C) C2H4O
D) CHO2
E) CH2O

Write a possible molecular formula for c4h4O.
A) C8H8O2
B) c12h12O2
C) c2h2o
D) C8H8O

What is the empirical formula for Hg2(NO3)2?
A) Hg2(NO3)2
B) hgno3
C) Hg(NO3)2
D) Hg2NO3
E) Hg4(NO3)4

Which of the following is an atomic element?
A) Br
B) H
C) N
D) O
E) Mg

Which of the following is a molecular element?
A) Kr
B) Ag
C) S
D) Mg
E) Ti

Which of the following is a molecular element?
A) Mg
B) Ar
C) Xe
D) I
E) Li

Which of the following is a molecular compound?
A) CuCl2
B) KCl
C) NaNO3
D) CH3Cl
E) RbBr

Which of the following is a molecular compound?
A) NaCN
B) LiOH
C) SrI2
D) ZnS
E) P4O10

Which of the following is an ionic compound?
A) LiCl
B) NO2
C) PCl3
D) CF4
E) SeBr2

Which of the following is an ionic compound?
A) SCl2
B) Mg3(PO4)2
C) Cl2O
D) CH2O
E) PF5

Write the formula for the compound formed between potassium and sulfur.
A) KS
B) KS2
C) K2S
D) K2SO3
E) K3S2

Give the name for SnO.
A) tin (I) oxide
B) tin (II) oxide
C) tin (III) oxide
D) tin (IV) oxide

Give the name for NaNO3.
A) sodium nitrite
B) sodium nitrate
C) sodium pernitrate
D) sodium hyponitrite
E) sodium hyponitrate

Write the formula for barium nitrite.
A) ba3n2
B) BaNO3
C) BN
D) Ba(NO2)2
E) B(NO2)3

Write the formula for strontium nitride.
A) Sr3N2
B) Sr(NO3)2
C) SrN
D) Sr2N3
E) Sr(NO2)2

Determine the name for TiCO3. Remember that titanium forms several ions.
A) titanium (II) carbonate
B) titanium carbide
C) titanium carbonite
D) titanium (II) carbonite
E) titanium (I) carbonate

Give the formula for sodium chlorate.
A) NaClO
B) NaClO2
C) NaClO3
D) NaClO4

Write the name for Sn(SO4)2. Remember that Sn forms several ions.
A) tin (I) sulfite
B) tin (IV) sulfate
C) tin sulfide
D) tin (II) sulfite
E) tin (I) sulfate

Determine the name for CoCl2?6H2O. Remember that Co forms several ions.
A) cobalt chloride hydrate
B) cobalt (I) chloride heptahydrate
C) cobalt (II) chloride heptahydrate
D) cobalt (II) chloride hexahydrate
E) cobalt (I) chloride

Write the name for Ca3(PO4)2.
A) calcium (III) phosphite
B) calcium (II) phosphite
C) calcium phosphate
D) tricalcium phosphorustetraoxide
E) calcium phosphite

Give the correct formula for aluminum sulfate.
A) Al22SO4
B) Al(SO4)3
C) Al3(SO4)2
D) Al2(SO4)3

Write the formula for copper (II) sulfate pentahydrate.
A) Cu2SO3?H5
B) Cu2S?H2O
C) CuS?5H2O
D) (CuSO4)5
E) CuSO4?5H2O

Determine the name for H2CO3.
A) carbonous acid
B) dihydrogen carbonate
C) carbonic acid
D) hydrocarbonic acid
E) hydrocarbide acid

Determine the name for aqueous HBr.
A) bromic acid
B) bromous acid
C) hydrobromous acid
D) hydrogen bromate
E) hydrobromic acid

Give the formula for sulfurous acid.
A) H2SO3
B) HSO3
C) H2SO4
D) HSO4

Identify the formula for nitric acid.
A) hno3
B) HNO2
C) HNO
D) HNO4

Determine the name for P4O10.
A) phosphorus (IV) oxide
B) diphosphorus pentoxide
C) phosphorus oxide
D) phosphorus (II) oxide
E) tetraphosphorus decoxide

Determine the name for N2O5.
A) dinitrogen pentoxide
B) nitrogen oxide
C) nitrogen (IV) oxide
D) nitrogen (II) oxide
E) nitrogen tetroxide

Determine the name for Cl2O.
A) chlorine oxide
B) dichlorine monoxide
C) chlorine (I) oxide
D) chlorine (II) oxide
E) chlorate

Determine the name for HClO3.
A) hydrochloric acid
B) hydrochlorus acid
C) chlorate acid
D) chloric acid
E) perchloric acid

Calculate the molar mass for Mg(ClO4)2.
A) 223.21 g/mol
B) 123.76 g/mol
C) 119.52 g/mol
D) 247.52 g/mol
E) 75.76 g/mol

Calculate the molar mass of Al(C2H3O2)3.
A) 86.03 g/mol
B) 204.13 g/mol
C) 56.00 g/mol
D) 258.09 g/mol
E) 139.99 g/mol

Calculate the molar mass of Ca3(PO4)2.
A) 87.05 g/mol
B) 215.21 g/mol
C) 310.18 g/mol
D) 279.21 g/mol
E) 246.18 g/mol

Calculate the molar mass of C8H6O4.
A) 166.13 g/mol
B) 182.09 g/mol
C) 150.18 g/mol
D) 172.13 g/mol

How many millimoles of Ca(NO3)2 contain 4.78 × 10^22 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164.10 g/mol.
A) 12.6 mmol Ca(NO3)2
B) 13.0 mmol Ca(NO3)2
C) 20.7 mmol Ca(NO3)2
D) 79.4 mmol Ca(NO3)2
E) 57.0 mmol Ca(NO3)2

How many moles of C3H8 contain 9.25 × 1024 molecules of C3H8?
A) 65.1 moles C3H8
B) 28.6 moles C3H8
C) 34.9 moles C3H8
D) 46.2 moles C3H8
E) 15.4 moles C3H8

How many N2O4 molecules are contained in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.
A) 5.54 × 10^25 N2O4 molecules
B) 7.26 × 10^23 N2O4 molecules
C) 1.38 × 10^24 N2O4 molecules
D) 4.59 × 10^25 N2O4 molecules
E) 4.99 × 10^23 N2O4 molecules

How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.05 g/mol.
A) 9.83 × 10^20 C2H4 molecules
B) 7.74 × 10^26 C2H4 molecules
C) 2.71 × 10^20 C2H4 molecules
D) 3.69 × 10^23 C2H4 molecules
E) 4.69 × 10^23 C2H4 molecules

What is the mass, in kg, of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol.
A) 3.85 kg
B) 5.04 kg
C) 2.60 kg
D) 3.03 kg
E) 6.39 kg

What is the mass of 9.44 × 1024 molecules of NO2? The molar mass of NO2 is 46.01 g/mol.
A) 205 g
B) 294 g
C) 721 g
D) 341 g
E) 685 g

Calculate the mass percent composition of sulfur in Al2(SO4)3.
A) 28.12%
B) 9.372%
C) 42.73%
D) 21.38%
E) 35.97%

Calculate the mass percent composition of lithium in Li3PO4.
A) 26.75%
B) 17.98%
C) 30.72%
D) 55.27%
E) 20.82%

How many moles of N2O3 contain 2.55 × 1024 oxygen atoms?
A) 1.41 moles N2O3
B) 4.23 moles N2O3
C) 12.7 moles N2O3
D) 7.87 moles N2O3
E) 2.82 moles N2O3

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?
A) 13.3 kg
B) 22.5 kg
C) 79.4 kg
D) 44.4 kg
E) 92.4 kg

Give the mass percent of carbon in C14H19NO2.
A) 38.89%
B) 72.07%
C) 5.17%
D) 2.78%

How many moles of PCl3 contain 3.68 × 1025 chlorine atoms?
A) 61.1 moles PCl3
B) 20.4 moles PCl3
C) 16.4 moles PCl3
D) 54.5 moles PCl3
E) 49.1 moles PCl3

How many moles of C3H8 contain 4.95 × 1024 hydrogen atoms?
A) 8.22 moles C3H8
B) 6.58 moles C3H8
C) 1.03 moles C3H8
D) 9.73 moles C3H8
E) 3.09 moles C3H8

How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.
A) 1.23 × 1023 O atoms
B) 2.96 × 1024 O atoms
C) 2.87 × 1025 O atoms
D) 1.10 × 1024 O atoms
E) 3.19 × 1024 O atoms

How many sodium ions are contained in 99.6 mg of Na2SO3? The molar mass of Na2SO3 is
126.05 g/mol.
A) 1.52 × 10^27 sodium ions
B) 4.76 × 10^20 sodium ions
C) 2.10 × 10^21 sodium ions
D) 1.05 × 10^21 sodium ions
E) 9.52 × 10^20 sodium ions

Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.
A) 8.59 mL
B) 13.5 mL
C) 7.40 mL
D) 12.4 mL
E) 11.6 mL

How many molecules 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.
A) 2.59 × 10^23 molecules butane
B) 1.46 × 10^27 molecules butane
C) 6.87 × 10^23 molecules butane
D) 1.56 × 10^23 molecules butane
E) 7.14 × 10^25 molecules butane

Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of c2h5o2.
A) C2H5O2
B) C6H15O6
C) C3H7O3
D) C4H10O4
E) C8H20O8

Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an empirical formula of NO2.
A) N2O3
B) N3O6
C) N2O4
D) NO2
E) N2O5

Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
A) NO
B) N2O
C) NO2
D) N2O3
E) NO3

Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl.
A) P3Cl
B) PCl
C) PCl2
D) P2Cl3
E) PCl3

Determine the empirical formula for a compound that contains C, H and O. It contains 51.59% C and 35.30% O by mass.
A) C2H6O
B) CHO
C) C4H13O2
D) CH4O3
E) CH3O

Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen.
A) C18H27NO3
B) C18H27NO2
C) C17H27NO3
D) C17H26NO3

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?
A) C5H2O
B) CHO
C) C3H6O
D) C3H7O
E) C6HO3

Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.
A) H2SO4(aq) + LiOH(aq) ? H2O(l) + Li2SO4(aq)
B) H2SO3(aq) + 2 LiOH(aq) ? 2 H2O(l) + Li2SO3(aq)
C) HSO3(aq) + LiOH(aq) ? H2O(l) + LiSO3(aq)
D) HSO4(aq) + LiOH(aq) ? H2O(l) + LiSO4(aq)
E) H2S(aq) + 2 LiOH(aq) ? 2 H2O(l) + Li2S(aq)

Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor.
A) 2 C2H6(g) + 7 O2(g) ? 4 CO2(g) + 6 H2O(g)
B) C2H6(g) + 5 O(g) ? 2 CO(g) + 3 H2O(g)
C) 2 C2H6(g) + 5 O2(g) ? 4 CO(g) + 6 H2O(g)
D) C2H6(g) + 7 O(g) ? 2 CO2(g) + 3 H2O(g)
E) 2 CH3(g) + 5 O(g) ? 2 CO(g) + 3 H2O(g)

Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) ? AlPO4(s) + 2 NH4C2H3O2(aq)
B) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) ? AlPO4(s) + 2 NH3C2H3O2(aq)
C) Al(CO3)2(aq) + (NH3)2PO4(aq) ? AlPO4(s) + 2 NH3CO3(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) ? AlPO4(s) + 3 NH4C2H3O2(aq)
E) Al(CO2)3(aq) + (NH4)3PO3(aq) ? AlPO3(s) + 3 NH4CO2(aq)

Which of the following is one possible form of pentane?
A) CH3CH2CH2CH2CH3
B) CH3CH=CHCH2CH3
C) CH3CH2CH2CH2CH2CH3
D) CH3CH2CH2CH2CH2NH2
E) CH3CH2-O-CH2CH2CH3

Identify the principal component of natural gas.
A) propane
B) ethane
C) n-butane
D) methane
E) n-pentane

Match the following.
A) I(s)
B) Cl(g)
C) O(g)
D) Cl2(g)
E) Ne2(g)
F) Ne(g)
G) Ca(s)
H) O2(g)
I) I2(s)
J) Ca2(s)

1) oxygen
2) chlorine
3) neon
4) calcium
5) iodine

How can one compound contain both ionic and covalent bonds? Give an example.

Describe the difference between a molecular formula and an empirical formula. Give an example.

Can you predict the chemical formula for a covalent compound between nitrogen and oxygen?

Describe the difference between an atomic element and a molecular element.

Describe the difference between ionic and molecular compounds. Give an example of each.

Why aren’t prefixes used in naming ionic compounds?

Give the name for HNO2.

Balance the following equation.
____ c10h12 + ____ O2 ? ____ H2O + ____ CO2

List the elements in a hydrocarbon.

In which set do all elements tend to form anions in binary ionic compounds?
A) C, S, Pb
B) K, Fe, Br
C) Li, Na, K
D) N, O, I

What type of bonding is found in the compound OF2?
A) covalent bonding
B) hydrogen bonding
C) ionic bonding
D) metallic bonding

Which one of the following compounds contains ionic bonds?
A) SrO
B) HBr
C) PBr3
D) SiO2

Which of the following is the correct chemical formula for a molecule of astatine?
A) At
B) At-
C) At+
D) At2

Which of the compounds, Li3N, NH3, C3H8, IF3 are ionic compounds?
A) only C3H8
B) only Li3N
C) Li3N and NH3
D) N H3, C3H8, and IF3

Which of the compounds C4H10, BaCl2, Ni(NO3)2, SF6 are expected to exist as molecular compounds?
A) only C4H10
B) C4H10 and SF6
C) C4H10, Ni(NO3)2, and SF6
D) BaCl2 and Ni(NO3)2

Which of the following elements has the least tendency to form an ion?
A) Ca
B) K
C) Kr
D) Se

In which set do all elements tend to form cations in binary ionic compounds?
A) K, Ga, O
B) Sr, Ni, Hg
C) N, P, Bi
D) O, Br, I

The solid compound, Na4SiO4, contains
A) Na+, Si4+, and O2- ions.
B) Na+ and SiO44- ions.
C) Na4+ and SiO44- ions.
D) Na4SiO4 molecules.

What is the chemical formula for iron(III) sulfate?
A) Fe3S
B) Fe3SO4
C) Fe2S3
D) Fe2(SO4)3

Rb2S is named
A) rubidium disulfide.
B) rubidium sulfide.
C) rubidium(II) sulfide.
D) rubidium sulfur.

What is the chemical formula for calcium hydroxide?
A) CaH2
B) CaOH
C) CaOH2
D) Ca(OH)2

What is the chemical formula for magnesium hydride?
A) MgH2
B) MgOH
C) MgOH2
D) Mg(OH)2

The chemical formula for lithium peroxide is
A) LiOH.
B) LiO2.
C) Li2O.
D) Li2O2.

The compound, Cu(N O2)2, is named
A) copper nitrite(II).
B) copper(I) nitrite.
C) copper(I) nitrite(II).
D) copper(II) nitrite.

The compound, ClO, is named
A) chlorite.
B) hypochlorite.
C) chlorine monoxide.
D) chlorine (II) oxide.

The chemical formula for calcium nitride is
A) Ca(NO3)2.
B) Ca(NO2)2.
C) Ca3N2.
D) CaN2.

An aqueous solution of H2S is named
A) hydrosulfuric acid.
B) hydrosulfurous acid.
C) sulfuric acid.
D) sulfurous acid.

The chemical formula for the sulfite ion is
A) S-.
B) S 2-.
C) SO32-.
D) SO42-.

The ion, IO2-, is named
A) iodate ion.
B) iodite ion.
C) iodine dioxide ion.
D) iodine(II) oxide ion.

The chemical formula for nitrous acid is
A) H3N(aq).
B) H NO2(aq).
C) H NO3(aq).
D) H2N2O6(aq).

What is the molar mass of nitrogen gas?
A) 14.0 g/mol
B) 28.0 g/mol
C) 6.02 × 1023 g/mol
D) 1.20 × 1023 g/mol

What is the mass of a single fluorine molecule, F2?
A) 3.155 × 10-23 g
B) 6.310 × 10-23 g
C) 19.00 g
D) 38.00 g

What is the mass of 0.500 mol of dichlorodifluoromethane, CCl2F2?
A) 4.14 × 10-3 g
B) 60.5 g
C) 121 g
D) 242 g

How many moles are there in 3.00 g of ethanol, CH3CH2OH?
A) 0.00725 mol
B) 0.0652 mol
C) 15.3 mol
D) 138 mol

What is the mass of 8.50 × 1022 molecules of NH3?
A) 0.00829 g
B) 0.417 g
C) 2.40 g
D) 121 g

What is the molar mass of 1-butene if 5.38 × 1016 molecules of 1-butene weigh 5.00 ?g?
A) 56.0 g/mol
B) 178 g/mol
C) 224 g/mol
D) 447 g/mol

What mass of carbon dioxide, CO2, contains the same number of molecules as 3.00 g of trichlorofluoromethane, CCl3F?
A) 0.106 g
B) 0.961 g
C) 1.04 g
D) 9.37 g

What mass of phosphorus pentafluoride, PF5, has the same number of fluorine atoms as 25.0 g of oxygen difluoride, OF2?
A) 0.933 g
B) 10.0 g
C) 23.3 g
D) 146 g

How many anions are there in 2.50 g of MgBr2?
A) 8.18 × 10^21 anions
B) 1.64 × 10^22 anions
C) 4.43 × 10^25 anions
D) 8.87 × 10^25 anions

Which of the following has the greatest mass?
A) 3.88 × 1022 molecules of O2
B) 1.00 g of O2
C) 0.0312 mol of O2
D) All of the above have the same mass.

Which of the following has the smallest mass?
A) 3.50 × 1023 molecules of I2
B) 85.0 g of Cl2
C) 2.50 mol of F2
D) 0.050 kg of Br2

The molecular weight of nitrous oxide (N2O), known as laughing gas, is ________ amu (rounded to one decimal place).
A) 60.0
B) 30.0
C) 44.0
D) 3.0
E) 22.0

A sample of pure lithium nitrate contains 10.1% lithium by mass. What is the % lithium by mass in a sample of pure lithium nitrate that has twice the mass of the first sample?
A) 5.05%
B) 10.1%
C) 20.2%
D) 40.4%

A sample of pure calcium fluoride with a mass of 15.0 g contains 7.70 g of calcium. How much calcium is contained in 40.0 g of calcium fluoride?
A) 2.27 g
B) 7.70 g
C) 15.0 g
D) 20.5 g

Which one of the following contains 39% carbon by mass?
A) C2H2
B) CH4
C) CH3NH2
D) CO2

Determine the mass percent (to the hundredths place) of H in sodium bicarbonate (NaHCO3).

What is the empirical formula of a compound that is 62.0% C, 10.4% H, and 27.5% O by mass?
A) C3HO
B) C6HO3
C) c6h12o2
D) c5h10o2
E) C3H6O

How many Fe(II) ions are there in 20.0 g of FeSO4?
A) 2.19 × 10^-25 iron(II) ions
B) 7.92 × 10^22 iron(II) ions
C) 4.57 × 10^24 iron(II) ions
D) 1.82 × 10^27 iron(II) ions

How many oxygen atoms are there in 7.00 g of sodium dichromate, Na2Cr2O7?
A) 0.187 oxygen atoms
B) 2.30 × 10^21 oxygen atoms
C) 1.60 × 10^22 oxygen atoms
D) 1.13 × 10^23 oxygen atoms

How many chloride ions are there in 4.50 mol of aluminum chloride?
A) 3.00 chloride ions
B) 13.5 chloride ions
C) 2.71 × 1024 chloride ions
D) 8.13 × 1024 chloride ions

How many cations are there in 10.0 g of sodium phosphate?
A) 3.67 × 1022 cations
B) 1.10 × 1023 cations
C) 9.87 × 1024 cations
D) 2.96 × 1025 cations

What is the empirical formula of a substance that contains 2.64 g of C, 0.444 g of H, and 3.52 g of O?
A) C H2O
B) C2H4O2
C) C2H4O3
D) c3h4o4

Which one of the following is not an empirical formula?
A) CHO
B) CH2O
C) C2H4O
D) C2H4O2

Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 0.80 g of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide?
A) 1.8 g
B) 2.2 g
C) 3.7 g
D) 4.0 g

Combustion analysis of an unknown compound containing only carbon and hydrogen produced 0.2845 g of CO2 and 0.1451 g of H2O. What is the empirical formula of the compound?
A) CH2
B) C2H5
C) C4H10
D) C5H2

Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?
A) C2H5O
B) C2H5O2
C) C2H10O3
D) C3H8O2

A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion of a 50.00 gram sample of the alcohol produced 95.50 grams of CO2 and 58.70 grams of H2O. What is the empirical formula of the alcohol?

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients?

_____ C2H6O(l) + _____ O2(g) ? _____ CO2(g) + _____ H2O(l)

A) 9
B) 7
C) 5
D) 3

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?
A) 1
B) 2
C) 3
D) 4

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered coefficients?
A) 1
B) 2
C) 3
D) none of these

Which of the following is a molecular element?
A) neon
B) lithium
C) selenium
D) magnesium
E) titanium

Identify the compound with covalent bonds.
A) CH4
B) Kr
C) KBr
D) Li
E) NaCl

Write the name for Sr3(PO4)2.
A) strontium (III) phosphite
B) strontium (II) phosphite
C) strontium phosphate
D) tristrontium phosphorustetraoxide
E) strontium phosphite

Which statement is true?
A) All chemical bonds share electrons between atoms.
B) A covalent bond involves transfer of electrons from a metal atom to a nonmetal atom.
C) An ionic bond involves transfer of electrons from a metal atom to a nonmetal atom.
D) An ionic bond is formed by sharing a pair of electrons.

What is the mass of a sample of water (H2O) containing 3.00 × 1022 H2O molecules?
A) 18.0 g
B) 0.900 g
C) 9.00 g
D) 1.00 mol

You are given three solid compounds (A, B, C) with melting temperatures 700°C, 150°C and 800°C respectively. Which of these is a molecular solid?
A) Solid A
B) Solid B
C) Solid C
D) Solids A, B, C

What is the coefficient for O2 when the equation is balance with smallest whole number coefficients?
_____ C4H10 + _____ O2 = _____ CO2 + _____ H2O
A) 13
B) 6.5
C) 1
D) 26

The mass of a He atom is ________.
A) 6.64 × 10^-24 g
B) 4.003 g
C) 2.40 × 10^24 g
D) 6.64 × 10^22 g

Vitamin E is a fat soluble vitamin with the formula C29H50O2 and a molar mass of 431 g/ mole. How many carbon atoms are in 30.0 mg?
A) 15.0 × 10^20
B) 4.10 × 10^20
C) 12.1 × 10^20
D) 4.20 × 10^22

How many atoms of oxygen are in 5.00 g of ethanol, C2H6O?
A) 6.52 × 10^22
B) 6
C) 5.52 × 10^24
D) 6.02 × 10^23

Calculate the moles of Fe in 16.0 g of Fe2O3.
A) 10.0 mol
B) 0.10 mol
C) 16.0 mol
D) 0.200 mol

Which has the least number of atoms?
A) 1mol O2
B) 1mol H2O
C) 4.0 g He
D) 1.2 g C