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WorksheetsStudent Activity - Ionic Bonding
Total questions: 150
Worksheet time: 1hrs 15mins
Define these terms: ionic bond. Choose the option that best states the definition.
Attraction between oppositely charged ions resulting from the transfer of electrons
Sharing of valence electrons equally between two nonmetals
A delocalized sea of electrons holding metal atoms together
Weak intermolecular forces between neutral molecules
Define these terms: lattice energy. Choose the option that best states the definition.
Energy given off when oppositely charged ions in the gas phase come together to form a solid lattice
Energy required to break covalent bonds within a molecular crystal
Energy stored in the motion of electrons within a metal lattice
Heat absorbed when a solid dissolves in water
Define these terms: salt. Choose the option that best states the definition.
An ionic compound formed from the electrostatic attraction between cations and anions
A covalent compound made of nonmetals sharing electrons
A pure metal consisting of identical atoms in a lattice
A polar molecule held together only by hydrogen bonds
Determine which of the following pairs has the greater lattice energy and therefore the stronger ionic bonds. Select the compound with the greater lattice energy: LiF or LiCl.
LiF
LiCl
Determine which of the following pairs has the greater lattice energy and therefore the stronger ionic bonds. Select the compound with the greater lattice energy: CaCl2 or MgCl2.
CaCl2
MgCl2
Determine which of the following pairs has the greater lattice energy and therefore the stronger ionic bonds. Select the compound with the greater lattice energy: MgO or Al2O3.
MgO
Al2O3
Determine which of the following pairs has the greater lattice energy and therefore the stronger ionic bonds. Select the compound with the greater lattice energy: Na2O or Na3N.
Na2O
Na3N
Lewis Dot Structures for Ionic Bonds: Choose the correct ion charges that result when LiF forms as an ionic compound.
Li+ and F−
Li2+ and F2−
Li− and F+
Li+ and F2−
Lewis Dot Structures for Ionic Bonds: Choose the correct ion charges that result when Na2O forms as an ionic compound.
two Na+ and O2−
Na+ and O−
Na2+ and O2−
two Na+ and O−
Lewis Dot Structures for Ionic Bonds: Choose the correct ion charges that result when BaO forms as an ionic compound.
Ba2+ and O2−
Ba+ and O−
Ba3+ and O3−
Ba2+ and O−
Lewis Dot Structures for Ionic Bonds: Choose the correct ion charges that result when CaCl2 forms as an ionic compound.
Ca2+ and two Cl−
Ca+ and Cl−
Ca2+ and Cl2−
Ca3+ and three Cl−
Lewis Dot Structures for Ionic Bonds: Choose the correct ion charges that result when K3N forms as an ionic compound.
three K+ and N3−
K+ and N−
K2+ and N2−
three K+ and N−
Find the formula of the ionic compound formed by Lithium and Fluorine. Write only the formula (no charges).
LiF
Li2F
LiF2
Li2F2
Find the formula of the ionic compound formed by Calcium and Sulfur. Write only the formula (no charges).
CaS
Ca2S
CaS2
Ca2S3
Find the formula of the ionic compound formed by Magnesium and Bromine (Br). Write only the formula (no charges).
MgBr2
Mg2Br
MgBr
Mg2Br3
Find the formula of the ionic compound formed by Strontium (Sr) and Phosphorous. Write only the formula (no charges).
Sr3P2
SrP2
Sr2P
SrP3
Find the formula of the ionic compound formed by Sodium and Sulfur. Write only the formula (no charges).
Na2S
NaS2
NaS
Na2S2
Find the formula of the ionic compound formed by Aluminum and Chlorine (Cl). Write only the formula (no charges).
AlCl3
Al3Cl
AlCl2
Al2Cl3
Find the formula of the ionic compound formed by Aluminum and Phosphorous. Write only the formula (no charges).
AlP
AlP3
Al3P
Al2P3
Find the formula for the ionic compound that contains polyatomic ions: sodium hydroxide.
NaOH
Na2OH
NaOH2
Na2O
Find the formula for the ionic compound that contains polyatomic ions: aluminum hydroxide.
Al(OH)3
AlOH3
Al2(OH)3
Al(OH)2
Find the formula for the ionic compound that contains polyatomic ions: lithium sulfate.
Li2SO4
LiSO4
Li2SO3
LiSO3
Find the formula for the ionic compound that contains polyatomic ions: calcium nitrate.
Ca(NO3)2
CaNO3
Ca2(NO3)2
Ca(NO2)2
Find the formula for the ionic compound that contains polyatomic ions: potassium phosphate.
K3PO4
KPO4
K2PO4
K3PO3
Find the formula for the ionic compound that contains polyatomic ions: lithium chlorate.
LiClO3
LiClO4
LiClO2
LiClO
Find the formula for the ionic compound that contains polyatomic ions: lithium perchlorate.
LiClO4
LiClO3
LiCl4O
LiClO2
Find the formula for the ionic compound that contains polyatomic ions: calcium perchlorate.
Ca(ClO4)2
CaClO4
Ca2(ClO4)2
Ca(ClO3)2
Find the formula for the ionic compound that contains polyatomic ions: ammonium fluoride (F−).
NH4F
NH4F2
(NH4)2F
NH3F
Find the formula for the ionic compound that contains polyatomic ions: ammonium acetate.
NH4C2H3O2
(NH4)2C2H3O2
NH4CH3CO3
NH3C2H3O2
Find the formula for the ionic compound that contains polyatomic ions: ammonium thiosulfate.
(NH4)2S2O3
NH4S2O3
(NH4)2SO3
(NH4)2S2O4
Name the following ionic compounds: NH4Cl
ammonium chloride
ammonium chlorate
ammonia chloride
nitrogen chloride
Name the following ionic compounds: Fe(NO3)3
iron(II) nitrate
iron(III) nitrate
iron(III) nitrite
iron(II) nitrite
Name the following ionic compounds: TiBr3
titanium(II) bromide
titanium(III) bromide
titanium(IV) bromide
titanium tribromide
Name the following ionic compounds: Cu3P
copper(II) phosphide
copper(I) phosphide
copper(III) phosphate
copper phosphate
Name the following ionic compounds: SnSe2
tin(II) selenide
tin(IV) selenide
tin(II) selenate
tin(IV) selenate
Name the following ionic compounds: GaAs
gallium arsenide
gallium(III) arsenate
gallium arsenite
gallium(II) arsenide
Name the following ionic compounds: CrSO4
chromium(III) sulfate
chromium(II) sulfite
chromium(II) sulfate
chromium(IV) sulfate
Name the following ionic compounds: Be(HCO3)2
beryllium bicarbonate
beryllium carbonate
beryllium hydrogen sulfate
beryllium hydroxide
Name the following ionic compounds: Mn2(SO4)3
manganese(II) sulfate
manganese(III) sulfate
manganese(IV) sulfate
manganese(III) sulfite
Name the following ionic compounds: Al(CN)3
aluminum cyanate
aluminum cyanide
aluminum(III) cyanate
aluminum carbide
Write the formulas for the following compounds: chromium (VI) phosphate
Cr3(PO4)2
Cr(PO4)2
Cr2(PO4)3
CrPO4
Write the formulas for the following compounds: vanadium (IV) carbonate
VCO3
V(CO3)2
V2(CO3)4
V2CO3
Write the formulas for the following compounds: tin (II) nitrate
SnNO3
Sn(NO3)2
Sn(NO2)2
Sn2(NO3)2
Write the formulas for the following compounds: cobalt (III) oxide
CoO
Co2O3
Co3O2
CoO2
Write the formulas for the following compounds: titanium (II) acetate
Ti(C2H3O2)2
TiC2H3O2
Ti2(C2H3O2)3
Ti(C2H3O2)3
Write the formulas for the following compounds: vanadium (V) sulfide
VS2
V2S5
V5S2
V2S3
Write the formulas for the following compounds: chromium (III) hydroxide
Cr(OH)2
Cr(OH)3
Cr2(OH)3
Cr3(OH)2
Write the formulas for the following compounds: lithium iodide
LiI
LiI2
Li2I
Li2I2
Write the formulas for the following compounds: lead (II) nitride
PbN2
Pb3N2
Pb2N3
PbN
Write the formulas for the following compounds: silver bromide
AgBr2
Ag2Br
AgBr
Ag2Br3
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: CaCO3
Calcium carbonate
Calcium chlorate
Calcium carbide
Calcium cyanide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: KCl
Potassium chlorate
Potassium chloride
Potassium perchlorate
Potassium chlorite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: FeSO4
Iron(II) sulfate
Iron(III) sulfate
Iron(II) sulfite
Iron(III) sulfite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: LiBr
Lithium bromide
Lithium bromate
Lithium bromite
Lithium peroxide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: MgCl2
Magnesium chlorate
Magnesium chloride
Magnesium chlorite
Magnesium perchlorate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: FeCl3
Iron(II) chloride
Iron(III) chloride
Iron(I) chloride
Iron(IV) chloride
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Zn3(PO4)2
Zinc(II) phosphate
Zinc(III) phosphate
Zinc phosphate
Zinc phosphite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: NH4NO3
Ammonium nitrate
Ammonium nitrite
Ammonium nitride
Ammonium nitric acid
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Al(OH)3
Aluminum oxide
Aluminum hydroxide
Aluminum hydroxyde
Aluminum hydride
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: CuC2H3O2
Copper(I) acetate
Copper(II) acetate
Copper(I) oxalate
Copper(II) oxalate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: PbSO3
Lead(II) sulfate
Lead(IV) sulfite
Lead(II) sulfite
Lead(IV) sulfate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: NaClO3
Sodium chlorate
Sodium chlorite
Sodium perchlorate
Sodium hypochlorite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: CaC2O4
Calcium carbonate
Calcium oxalate
Calcium acetate
Calcium chromate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Fe2O3
Iron(II) oxide
Iron(III) oxide
Iron(I) oxide
Iron(IV) oxide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: (NH4)3PO4
Ammonium phosphate
Ammonium phosphite
Ammonium phosphide
Ammonium peroxide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: NaHSO4
Sodium sulfate
Sodium hydrogen sulfate
Sodium sulfite
Sodium bisulfite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Hg2Cl2
Mercury(II) chloride
Mercury(I) chloride
Mercury(III) chloride
Mercury(I) chlorate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Mg(NO3)2
Magnesium nitrite
Magnesium nitrate
Magnesium nitride
Magnesium nitric acid
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: CuSO4
Copper(I) sulfate
Copper(II) sulfate
Copper(I) sulfite
Copper(III) sulfate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: NaHCO3
Sodium hydrogen carbonate
Sodium carbonate
Sodium bicarbonate (acid salt)
Sodium hydrogencarbonate
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: NiBr3
Nickel(II) bromide
Nickel(III) bromide
Nickel(I) bromide
Nickel(IV) bromide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: Be(NO3)2
Beryllium nitrate
Beryllium nitrite
Beryllium nitride
Beryllium nitric acid
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: ZnSO4
Zinc sulfite
Zinc sulfate
Zinc(III) sulfate
Zinc(II) sulfide
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: AuClO3
Gold(III) chlorate
Gold(II) chlorate
Gold(I) chlorate
Gold(I) chlorite
Naming Ionic Compounds: Name each compound using the Stock Naming System. Compound: KMnO4
Potassium manganate
Potassium permanganate
Potassium manganite
Potassium perchlorate
Writing Formulas from Names: Write the formula of each compound. Name: ammonium phosphate
(NH4)3PO4
NH4PO4
(NH4)2PO4
NH4(PO4)2
Writing Formulas from Names: Write the formula of each compound. Name: iron(II) oxide
Fe2O3
FeO
Fe2O
Fe(OH)2
Writing Formulas from Names: Write the formula of each compound. Name: iron(III) oxide
FeO
Fe3O2
Fe2O3
FeO2
Writing Formulas from Names: Write the formula of each compound. Name: carbon monoxide
CO2
C2O
CO
C2O2
Writing Formulas from Names: Write the formula of each compound. Name: calcium chloride
CaCl2
Ca2Cl
CaCl
Ca2Cl2
Writing Formulas from Names: Write the formula of each compound. Name: potassium nitrate
KNO2
KNO3
K2NO3
K(NO3)2
Writing Formulas from Names: Write the formula of each compound. Name: magnesium hydroxide
MgOH
Mg(OH)2
Mg(OH)3
Mg2(OH)2
Writing Formulas from Names: Write the formula of each compound. Name: aluminum sulfate
Al2(SO4)3
Al(SO4)2
AlSO4
Al2SO4
Writing Formulas from Names: Write the formula of each compound. Name: copper(II) sulfate
CuSO3
Cu(SO4)2
CuSO4
Cu2SO4
Writing Formulas from Names: Write the formula of each compound. Name: lead(IV) chromate
PbCrO4
Pb(CrO4)2
Pb2CrO4
Pb(CrO4)4
Writing Formulas from Names: Write the formula of each compound. Name: diphosphorus pentoxide
P2O5
P5O2
P2O3
PO5
Writing Formulas from Names: Write the formula of each compound. Name: potassium permanganate
KMnO4
K2MnO4
KMnO3
K(MnO4)2
Writing Formulas from Names: Write the formula of each compound. Name: sodium hydrogen carbonate
NaHCO3
Na2CO3
NaHCO2
NaHCNO3
Writing Formulas from Names: Write the formula of each compound. Name: zinc nitrate
Zn(NO3)2
Zn(NO2)2
Zn2(NO3)2
ZnNO3
Writing Formulas from Names: Write the formula of each compound. Name: aluminum sulfite
Al2(SO3)3
Al2(SO4)3
Al(SO3)2
Al2SO3
Practice: Determine the molar mass for the compound calcium bromide, CaBr2. Select the correct molar mass in g/mol.
199.886 g/mol
214.904 g/mol
119.902 g/mol
159.912 g/mol
Practice: Determine the molar mass for the compound sodium sulfate, Na2SO4. Select the correct molar mass in g/mol.
142 g/mol
118 g/mol
174 g/mol
126 g/mol
Practice: Determine the molar mass for the compound calcium nitrite, Ca(NO2)2. Select the correct molar mass in g/mol.
132.052 g/mol
164.088 g/mol
118.086 g/mol
148.096 g/mol
Practice: Determine the molar mass for the compound ammonium phosphate, (NH4)3PO4. Select the correct molar mass in g/mol.
149.087 g/mol
121.970 g/mol
167.051 g/mol
138.204 g/mol
Name each compound below and calculate the molar mass: For Fe2O3, choose the correct compound name and molar mass pair.
Iron(III) oxide; 159.687 g/mol
Iron(II) oxide; 143.691 g/mol
Iron(III) oxide; 175.690 g/mol
Iron(II) oxide; 159.687 g/mol
Name each compound below and calculate the molar mass: For K2CO3, choose the correct compound name and molar mass pair.
Potassium carbonate; 138.204 g/mol
Potassium bicarbonate; 100.115 g/mol
Potassium carbonate; 122.103 g/mol
Potassium oxide; 94.196 g/mol
Name each compound below and calculate the molar mass: For Al(NO3)3, choose the correct compound name and molar mass pair.
Aluminum nitrate; 212.994 g/mol
Aluminum nitrite; 212.994 g/mol
Aluminum nitrate; 88.986 g/mol
Aluminum nitride; 40.988 g/mol
Name each compound below and calculate the molar mass: For Cu(C2H3O2)2, choose the correct compound name and molar mass pair.
Copper(II) acetate; 181.634 g/mol
Copper(I) acetate; 181.634 g/mol
Copper(II) nitrate; 187.554 g/mol
Copper(II) acetate; 159.687 g/mol
Complete the following mol conversion using dimensional analysis: What is the mass of 4.68 moles of iron(III) oxide, Fe2O3? Select the correct mass in grams.
747.34 g
587.00 g
212.99 g
181.63 g
Complete the following mol conversion using dimensional analysis: How many moles are in 587 g of aluminum nitrate, Al(NO3)3? Select the correct number of moles.
2.76 mol
1.55 mol
4.68 mol
0.50 mol
Complete the following mol conversion using dimensional analysis: What is the mass of 1.55 mol of copper(II) acetate, Cu(C2H3O2)2? Select the correct mass in grams.
281.53 g
138.20 g
159.69 g
212.99 g
Complete the following mol conversion using dimensional analysis: Calculate the number of moles in 0.500 g of potassium carbonate, K2CO3. Select the correct number of moles.
0.00360 mol
0.0360 mol
0.000360 mol
0.00600 mol
Evaluate the molar mass using the expression (55.845)+(3×35.45) and choose the correct value in g/mol.
162.195 g/mol
161.285 g/mol
166.195 g/mol
158.345 g/mol
Evaluate the molar mass using the expression (12.011)+(2×35.35)+(2×18.998) and choose the correct value in g/mol.
120.707 g/mol
118.711 g/mol
122.705 g/mol
126.699 g/mol
Evaluate the molar mass using the expression (238.03)+(6×18.998) and choose the correct value in g/mol.
352.018 g/mol
349.035 g/mol
360.028 g/mol
340.018 g/mol
Evaluate the molar mass using the expression (3×1.008)+(30.974)+(4×15.999) and choose the correct value in g/mol.
97.994 g/mol
95.986 g/mol
101.004 g/mol
99.992 g/mol
Evaluate the molar mass using the expression (2×12.011)+(4×1.008)+(2×15.999) and choose the correct value in g/mol.
60.052 g/mol
58.036 g/mol
62.060 g/mol
64.048 g/mol
Evaluate the molar mass using the expression (2×69.723)+(3×32.06)+(9×15.999) and choose the correct value in g/mol.
379.617 g/mol
367.601 g/mol
389.627 g/mol
371.609 g/mol
Given the following, find the number of moles: 30 grams of H3PO4.
0.31 moles
0.98 moles
3.3 moles
0.03 moles
Given the following, find the number of moles: 25 grams of HF.
0.25 moles
1.25 moles
2.50 moles
0.05 moles
Given the following, find the number of moles: 110 grams of NaHCO3.
0.84 moles
1.31 moles
2.44 moles
0.11 moles
Given the following, find the number of moles: 1.1 grams of FeCl3.
0.0068 moles
0.068 moles
0.11 moles
0.0011 moles
Given the following, find the number of moles: 987 grams of Ra(OH)2.
0.38 moles
2.60 moles
3.79 moles
9.87 moles
Given the following, find the number of moles: 564 grams of copper.
0.64 moles
5.64 moles
8.88 moles
56.4 moles
Given the following, find the number of moles: 12.3 grams of CO2.
0.28 moles
1.23 moles
2.44 moles
0.044 moles
Given the following, find the number of moles: 89 grams of Pb(CH3COO)4.
0.020 moles
0.20 moles
2.0 moles
0.89 moles
Given the following, find the number of grams: 4 moles of Cu(CN)2.
115.6 g
231.2 g
462.3 g
923.0 g
Given the following, find the number of grams: 5.6 moles of C6H6.
78.1 g
218.7 g
437.4 g
781.1 g
Given the following, find the number of grams: 21.3 moles of BaCO3.
420 g
4,203 g
420,300 g
197 g
Given the following, find the number of grams: 1.2 moles of (NH4)3PO3.
133.1 g
146.4 g
159.7 g
172.0 g
Given the following, find the number of grams: 9.3×103 moles of SmO.
1.55 × 10^4 g
1.55 \times 10^5 g
1.55 × 10^6 g
1.55 × 10^7 g
Given the following, find the number of grams: 6.6 moles of ZnO.
81.4 g
330.9 g
537.1 g
813.8 g
Given the following, find the number of grams: 5.4 moles of K2SO4.
472 g
706 g
941 g
1,174 g
Given the following, find the number of grams: 88.4 moles of NI3.
3,489 g
34,892 g
348,920 g
3,489,200 g
In the two hydrogen atoms simulation, which best describes what happens to the electrons and forces as the atoms move close together and then are pushed too close?
As the atoms approach, each nucleus attracts the other atom’s electron, lowering potential energy; if pushed too close, repulsion between like charges dominates and increases potential energy.
As the atoms approach, electrons stop moving and forces cancel; if pushed too close, attraction continues to increase with no repulsion.
As the atoms approach, only electron–electron repulsion occurs, raising potential energy; if pushed too close, attraction suddenly appears and lowers potential energy.
As the atoms approach, forces remain unchanged; if pushed too close, the bond breaks due to gravity.
Can one atom in a covalent bond win the "tug of war" for the shared electrons, and what would that imply for the bond?
No; the atoms share the pair of electrons and neither fully takes them, so the bond remains covalent.
Yes; one atom takes both electrons completely, creating a stronger covalent bond.
Yes; one atom loses both electrons, forming a metallic bond.
No; if one atom won, the bond would become ionic with electron transfer, which does not happen in a covalent bond.
What is a covalent bond?
An electrostatic attraction between cations and anions after electron transfer
An attraction between a metal lattice and a sea of mobile electrons
A shared pair of electrons attracting two atomic nuclei
A force caused by gravitational attraction between atoms
Which type of elements most commonly form covalent bonds?
Metals with metals
Metals with nonmetals
Nonmetals with nonmetals
Noble gases with alkali metals
In terms of electronegativity, why does hydrogen behave differently from other elements in its group when it comes to bonding?
Hydrogen has very high electronegativity for its period, so gaining an electron can make it stable like helium, while losing one makes it highly unstable.
Hydrogen has the lowest electronegativity in the periodic table, so it always loses electrons to form cations.
Hydrogen has the same electronegativity as alkali metals, so it always transfers its electron to form ionic bonds.
Hydrogen’s electronegativity prevents it from forming any bonds at all.
Why do nonmetals tend to be good at sharing electrons in covalent bonds?
They have nearly full valence shells and can achieve a full octet by sharing electrons.
They have empty valence shells and prefer to lose electrons.
They possess mobile electrons that delocalize through a lattice.
They are too large to attract electrons strongly.
In the potential energy simulation, why does the potential energy between two atoms decrease as you move them closer together (before they are too close)?
Each nucleus attracts the other atom’s electron, strengthening the attraction and lowering potential energy.
Only electron–electron repulsion is increasing, which lowers potential energy.
The nuclei lose mass as they approach, lowering energy.
Gravitational forces overcome electric forces at short range.
In the potential energy simulation, after a certain point the potential energy increases if you try to move the atoms any closer. Why does this happen?
Nucleus–nucleus and electron–electron repulsions dominate at very short distances, raising potential energy.
Electron sharing stops and the atoms become neutral, raising potential energy.
Only nucleus–electron attraction increases, raising potential energy.
Magnetic forces cancel all attractions.
What determines the bond length of a covalent bond?
The distance at which the potential energy of the two atoms is at a minimum
The smallest possible distance two atoms can touch without overlapping
The average atomic radius of the two atoms added together
The number of isotopes present in the sample
In terms of stability, why do atoms form covalent bonds?
To gain, share, or count electrons toward a filled valence shell and become more stable
To maximize the number of unpaired electrons
To decrease nuclear charge
To reduce electronegativity to zero
In the formula H–H, what does the line represent?
One shared pair of electrons between the two hydrogen atoms
A dashed bond indicating weak attraction
A notation for electron transfer from one H to the other
A depiction of two pairs of shared electrons
How many pairs of electrons does each oxygen atom share in an O2 molecule?
One pair
Two pairs
Three pairs
Four pairs
Using lines to represent bonds, how is the bond between two oxygen atoms in O2 depicted?
A single line between the atoms
Two lines between the atoms
Three lines between the atoms
No line between the atoms
How many electrons in total are shared in a triple bond?
2
4
6
8
Triple bonds are strongest, followed by double bonds, and single bonds are weakest. Which choice best explains this trend using electric force?
More shared electrons increase the electrostatic attraction between nuclei and the shared electron density, strengthening the bond.
Fewer shared electrons produce more repulsion, strengthening the bond.
Electrostatic forces are weaker when more electrons are shared, weakening the bond.
Bond strength is unrelated to electrostatic forces.
Name the covalent compound with the formula N2O.
Dinitrogen monoxide
Nitrogen dioxide
Dinitrogen trioxide
Nitrogen monoxide
Name the covalent compound with the formula NO2.
Nitrogen dioxide
Dinitrogen monoxide
Nitrogen monoxide
Dinitrogen dioxide
Name the covalent compound with the formula N2O4.
Dinitrogen tetraoxide
Dinitrogen trioxide
Nitrogen tetroxide
Nitrogen dioxide
Name the covalent compound with the formula N2O3.
Dinitrogen trioxide
Nitrogen trioxide
Dinitrogen dioxide
Nitrogen monoxide
Name the covalent compound with the formula NO.
Nitrogen monoxide
Dinitrogen monoxide
Nitrogen dioxide
Dinitrogen dioxide
Name the covalent compound with the formula H2O.
Water (dihydrogen monoxide)
Hydrogen oxide (monohydrogen dioxide)
Dihydrogen oxide(II)
Hydrogen(II) oxide trihydrate
Name the covalent compound with the formula S2O.
Disulfur monoxide
Sulfur monoxide
Sulfur dioxide
Disulfur dioxide
Name the covalent compound with the formula SO3.
Sulfur trioxide
Sulfur dioxide
Disulfur trioxide
Sulfur monoxide
Name the covalent compound with the formula S2O3.
Disulfur trioxide
Sulfur trioxide
Disulfur monoxide
Disulfur dioxide
Name the covalent compound with the formula SO2.
Sulfur dioxide
Sulfur monoxide
Sulfur trioxide
Disulfur dioxide
Name the covalent compound with the formula S2Cl2.
Disulfur dichloride
Sulfur chloride
Disulfur trichloride
Sulfur dichloride
