6.E: Exercises
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Matching: Identify each of the following as a cation, anion, or neutral atom. You can use the build atom PhET simulation to practice.
a. 
b. 
c. 
d. 
Matching: Match the following bond feature with the correct type of bond (ionic or covalent):
a. Transfer of electrons
b. Sharing of electrons
c. Involves molecules only
d. Involves ions only
e. Metals present
The charge of an ion with 13 protons and 11 electrons is?
a. 1+
b. 2+
c. 3+
d. 4+
The charge of an ion with 12 protons and 10 electrons is?
a. 1+
b. 2+
c. 3+
d. 4+
Which of the following atoms would lose electrons to other atoms when they form ionic bonds (check all that apply)?
a. \(\ce{Mg}\)
b. \(\ce{Cl}\)
c. \(\ce{O}\)
d. \(\ce{Li}\)
e. \(\ce{S}\)
Which of the following atoms would form covalent bonds (check all that apply)?
a. \(\ce{Mg}\)
b. \(\ce{Cl}\)
c. \(\ce{O}\)
d. \(\ce{Li}\)
e. \(\ce{S}\)
Match the formula and symbol of an ion with each of the following descriptions:
a. 13 protons and 10 electrons: __________
b. 13 protons and 13 electrons: __________
c. 14 protons and 14 electrons: __________
d. 15 protons and 15 electrons: __________
e. 15 protons and 18 electrons: __________
Fill in each blank with a suitable one word:
a. When an atom gains electron(s) an ion with a _______ charge is formed.
b. When an atom loses electron(s) an ion with a _______ charge is formed.
c. Elements in group 1A form ions by (losing/gaining) ______ a total of ______ electrons.
d. Elements in group 3A form ions by (losing/gaining) ______ a total of ______ electrons.
e. Elements in group 5A form ions by (losing/gaining) ______ a total of ______ electrons.
f. Elements in group 7A form ions by (losing/gaining) ______ a total of ______ electrons.
How many protons and electrons are in each of the following ions?
\(\ce{Sr^{2+}}\): __________
\(\ce{Cl^{-}}\): __________
\(\ce{As^{3+}}\): __________
Ionic Compounds
In ionic compounds lose their valence electrons to form positively charged ________.
a. Metals; anions
b. Nonmetals; cations
c. Metals; polyatomic ions
d. Nonmetals; anions
e. Metals; cations
Which of the following is the correct formula for the ion that would form between calcium and phosphorous? (Hint: you must first figure out the ionic charge for each).
a. \(\ce{CaP}\)
b. \(\ce{Ca2P}\)
c. \(\ce{Ca3P}\)
d. \(\ce{Ca3P2}\)
e. \(\ce{Ca2P3}\)
Lithium carbonate is used in the treatment of bipolar disorder. What is the chemical formula of lithium carbonate?
a. \(\ce{LiCO}\)
b. \(\ce{Li2CO3}\)
c. \(\ce{Li(CO3)2}\)
d. \(\ce{Li2CO}\)
Which of the following is the correct formula for the ion that would form between iron(III) and sulfur? (Hint: you must first figure out the ionic charge for each).
a. \(\ce{FeS}\)
b. \(\ce{Fe3S}\)
c. \(\ce{Fe2S3}\)
d. \(\ce{Fe3S2}\)
e. \(\ce{Fe(III)S2}\)
An ionic compound is formed from the interaction of a ______ and ______.
Is \(\ce{NH4Cl}\) ionic compound or molecular compound?
Although all atoms in \(\ce{NH4Cl}\) are nonmetal, \(\ce{NH4Cl}\) is ionic compound. What is the reason?
Although \(\ce{NH4Cl}\) is an ionic compound, we can find covalent bonds in this compound. How is it possible for covalent bond exist in an ionic compound?
Select all that apply. Which of the following combinations can likely interact to form an ionic compound.
a. Sodium and potassium
b. Lithium and calcium
c. Oxygen and nitrogen
d. Calcium and nitrogen
e. Sodium and oxygen
f. Carbon and chlorine
What is the charge of the cation in \(\ce{TiO2}\)?
a. 2+
b. 2-
c. 4+
d. 4-
What is the charge of the cation in \(\ce{MnO2}\)?
a. 2+
b. 2-
c. 4+
d. 4-
What is the charge of the cation in \(\ce{FeO}\)?
a. 2+
b. 2-
c. 4+
d. 4-
What is the charge of the cation in \(\ce{SrO}\)?
a. 2+
b. 2-
c. 4+
d. 4-
What is the charge of the cation in \(\ce{Fe2O3}\)?
a. 2-
b. 2+
c. 3+
d. 3-
Naming, Writing Ionic formulas
Consider the elements sulfur and potassium.
a. Identify each as a metal or a nonmetal.
b. State the number of valence electrons for each.
c. State the number of electrons that must be lost or gained for each to achieve an octet.
d. Write the symbol, including its ionic charge, and the name for each ion.
Write the symbols for the ions and the correct formula for the ionic compound that would form when each of the following react:
a. calcium and oxygen
b. magnesium and phosphorus
Write the name for each of the following compounds:
a. \(\ce{Mn2S3}\)
b. \(\ce{SnF4}\)
c. \(\ce{Cu2O}\)
d. \(\ce{Cr2O3}\)
e. \(\ce{TiO2}\)
What is the name of the cation in \(\ce{FeO}\)? __________
What is the name of the cation in \(\ce{TiO2}\)? __________
The correct formula for a compound comprised of \(\ce{Fe^{3+}}\) and sulfur is: __________
Write chemical formulas for the following compounds:
a. Lithium oxide: __________
b. Zinc bromide: __________
c. Iron (III) sulfide: __________
Name the following ionic compounds:
a. \(\ce{MnCl3}\): __________
b. \(\ce{PbO2}\): __________
c. \(\ce{KCl}\): __________
Provide a systematic name for each of the following compounds
a. \(\ce{Al2S3}\): __________
b. \(\ce{CaO}\): __________
c. \(\ce{Ba3P2}\): __________
d. \(\ce{NaBr}\): __________
e. \(\ce{Na3P}\): __________
f. \(\ce{NH4NO3}\): __________
g. \(\ce{Ca3(PO4)2}\): __________
h. \(\ce{Fe2(CO3)_3}\): __________
i. \(\ce{PbO}\): __________
j. \(\ce{PbO2}\): __________
Polyatomic Ions
In some ionic compounds, when a metal can form two or more types of ions, we cannot predict the __________ from the group number. Therefore, a roman numeral that is equal to the __________ is placed in parentheses immediately after the name of the metal, for example, \(\ce{Fe^{2+}}\) is called iron(II).
Matching: Match the polyatomic formula to its correct name from the list: phosphate, carbonate, sulfate, ammonium, sulfite.
a. \(\ce{SO^{2-}_3}\): __________
b. \(\ce{CO^{2-}_3}\): __________
c. \(\ce{SO^{2-}_4}\): __________
d. \(\ce{PO^{3-}_4}\): __________
e. \(\ce{NH^{1+}_4}\): __________
Aluminum hydroxide present in antacid is used in Mylanta to treat acid indigestion. Identify the polyatomic ion present in this particular antacid.
a. \(\ce{SO^{2-}_4}\)
b. \(\ce{OH^{-}}\)
c. \(\ce{AlOH^{2-}}\)
d. \(\ce{ClO^{-}_4}\)
e. None of these
The correct name of the compound comprised of \(\ce{Gd^{3+}}\) and \(\ce{SO_3^{2-}}\) is:
a. Gold (III) sulfide
b. Gold sulfate
c. Gold (III) sulfite
d. Gadolinium sulfite
e. Gadolinium sulfate
Match the following polyatomic ions with their corresponding names.
| Polyatomic ions | Names |
|---|---|
|
a. \(\ce{OH-}\) b. \(\ce{NO2-}\) c. \(\ce{NO3-}\) d. \(\ce{NH4+}\) e. \(\ce{CO3^{2-}}\) f. \(\ce{PO4^{3-}}\) g. \(\ce{PO3^{3-}}\) h. \(\ce{SO4^{2-}}\) |
Phosphite Carbonate Phosphate Sulfate Hydroxide Nitrate Ammonium Nitrite |
Write the formula for a compound containing the following:
a. ammonium ions and phosphate ions
b. iron (III) ions and bicarbonate ions
Name each of the following compounds:
a. \(\ce{Al(OH)3}\): __________
b. \(\ce{Cu(NO2)2}\): __________
c. \(\ce{KClO3}\): __________
d. \(\ce{Co3(PO4)2}\): __________
e. \(\ce{SrSO3}\): __________
Naming and Writing Covalent formulas
Name the following molecular compounds:
a. \(\ce{NCl3}\): __________
b. \(\ce{SiBr4}\): __________
c. \(\ce{Br2O}\): __________
d. \(\ce{S3N2}\): __________
Write the formula for each of the following molecular compounds:
a. iodine pentafluoride: __________
b. carbon diselenide: __________
c. diboron trioxide: __________
Write the formula for the molecular compound dinitrogen pentoxide: __________
Classify each of the following compounds as ionic or molecular:
a. \(\ce{LiH2PO4}\)
b. \(\ce{ClF3}\)
c. \(\ce{Mg(ClO2)}\)
d. \(\ce{NI3}\)
e. \(\ce{Ca(HSO3)2}\)
Name the following compounds:
a. \(\ce{CS2}\): __________
b. \(\ce{PBr3}\): __________
c. \(\ce{N2O3}\): __________
d. \(\ce{CCl4}\): __________
e. \(\ce{N2O}\): __________
f. \(\ce{SO3}\): __________
Write the formula for each of the following compounds:
a. Phosphorus pentachloride
b. Dichlorine oxide
c. Dinitrogen difluoride
d. Sulfur hexafluoride
e. Nitrogen triiodide
f. Silicon tetrachloride
Write the formula for each of the following compounds:
a. Phosphorus trichloride
b. Dichlorine Heptoxide
c. Nitrogen Dioxide
d. Xenon Tetrafluoride
e. Sulfur Trioxide
f. Carbon Monoxide
Naming, Writing Ionic, Covalent formulas
| Compound | Name |
|---|---|
| \(\ce{MnSO4}\) | |
| Diphosphorous tetraoxide | |
| Nitrous acid | |
| \(\ce{Al(HCO3)3}\) | |
| \(\ce{Ca3N2}\) | |
| Phosphoric acid | |
| \(\ce{H2S}\) | |
| Aluminum oxide | |
| \(\ce{P2Br8}\) | |
| \(\ce{CaCl2}\) | |
| \(\ce{H2CO3}\) | |
| Barium phosphate | |
| Cobalt (II) nitrate | |
| Pentanitrogen heptachloride | |
| Hydrofluoric acid | |
| ammonium phosphide | |
| Titanium (IV) phosphide | |
| Copper (II) nitrate hexahydrate |
Molecular Compounds and Lewis Structures
(Multi select) In the list below, select the elements that do not exist as diatomic molecules:
a. Hydrogen
b. Carbon
c. Nitrogen
d. Oxygen
e. Sulfur
f. Chlorine
(Multi select) In the list below, select the elements that do exist as diatomic molecules:
a. Iodine
b. Chlorine
c. Phosphorus
d. Hydrogen
e. Bromine
f. Magnesium
State the number of valence electrons, bonding pairs, and lone pairs in the following Lewis structure:
Valence electrons: __________
Bonding pairs: __________
Lone pairs: __________
Benzene is a colorless molecular compound commonly used in the United States and known to cause cancer. Determine the molecular formula of the benzene molecule based on structural formula below: (black = \(\ce{C}\), white = \(\ce{H}\), yellow = \(\ce{S}\), green = \(\ce{Cl}\)).
a. \(\ce{C3H4O}\)
b. \(\ce{C3H4O6}\)
c. \(\ce{C3H4}\)
d. \(\ce{C6H6}\)
How many valence electrons are present in the molecule \(\ce{SCl6}\)?
a. 48
b. 42
c. 118
d. 34
Electronegativity and Bond Polarity
Identify the more polar bond in each pair below.
a. \(\ce{HF}\) or \(\ce{HCl}\)
b. \(\ce{NO}\) or \(\ce{CO}\)
c. \(\ce{SH}\) or \(\ce{OH}\)
d. \(\ce{CN}\) or \(\ce{NN}\)
The most non-polar bond in the molecule shown below is:
a. \(\ce{O-H}\)
b. \(\ce{C-O}\)
c. \(\ce{C-Cl}\)
d. \(\ce{C-Br}\)
e. \(\ce{C-H}\)
What is the trend of electronegativity on a periodic table?
a. Electronegativity decreases from left to right across a period
b. Electronegativity increases from left to right across a period
c. Electronegativity increases down the group
d. Electronegativity does not vary within a group
What is the most electronegative element on the periodic table? __________
Which of the following elements are arranged in order of increasing electronegativity from left to right?
a. \(\ce{F, N, O, C}\)
b. \(\ce{Mg, Cl, Si, C}\)
c. \(\ce{Al, P, S, Cl}\)
d. \(\ce{P, Br, O, Cl}\)
Shapes and Polarity of Molecules
Below is the structure of acetyl chloride, drawn with bonds and electron dots. Will acetyl chloride dissolve in ethanol a polar solvent?
a. Yes, because acetyl chloride is a non-polar molecule
b. Yes, because acetyl chloride is a polar molecule
c. No because acetyl chloride is a non-polar molecule
d. No because acetyl chloride is an ionic compound
Draw the Lewis-dot structures for each of the compounds listed below, then match the specified atom in each structure with the correct electron-group arrangement and molecular shape (please refer to your text for electron-group arrangements and molecular shapes).
Example: For oxygen in \(\ce{H2O}\), the molecular shape is bent, and the electron-group arrangement is tetrahedral.
| The oxygen atom in \(\ce{H3COH}\) |
Electron-group: __________ Molecular shape: __________ |
| The boron atom in \(\ce{BCl3}\) |
Electron-group: __________ Molecular shape: __________ |
| The nitrogen atom in \(\ce{NH3}\) |
Electron-group: __________ Molecular shape: __________ |
| The carbon atom in \(\ce{CF4}\) |
Electron-group: __________ Molecular shape: __________ |
| The carbon atom in \(\ce{CO2}\) |
Electron-group: __________ Molecular shape: __________ |
Fill in the blank or Matching: Complete each of the following statements for a molecule of \(\ce{CF4}\):
a. The number of electron groups around the central atom ________.
b. The electron geometry ________.
c. The number of carbon atoms attached to the central \(\ce{C}\) is: ________.
d. The shape of the molecule is
Use the molecule polarity simulation to observe the dipoles of \(\ce{HCN}\) and determine which element is the most electronegative
a. \(\ce{H}\)
b. \(\ce{C}\)
c. \(\ce{N}\)
Use the molecule polarity simulation to determine whether each of these compounds are polar or non-polar:
a. \(\ce{CF4}\): __________
b. \(\ce{HF}\): __________
c. \(\ce{CH2O}\): __________
d. \(\ce{H2O}\): __________
e. \(\ce{CHF3}\): __________
Select the number of electron groups and lone pairs and use VSEPR theory to determine the shape of \(\ce{PF3}\).
a. 4 electron groups, 1 lone pair, trigonal pyramidal
b. 4 electron groups, 2 lone pairs, bent
c. 3 electron groups, no lone pairs, trigonal planar
d. 3 electron groups, 1 lone pair, bent
Attractive Forces in Compounds
Match the boiling points (100 \(^{\circ}\)C, 1935 \(^{\circ}\)C, -34.6 \(^{\circ}\)C, 76.72 \(^{\circ}\)C)
a. \(\ce{H2O}\)
b. \(\ce{CaCl2}\)
c. \(\ce{Cl2}\)
d. \(\ce{CCl4}\)
Rank the following molecules from least (1) to highest (4) in terms of the strength of their intermolecular forces: \(\ce{H2S}\), \(\ce{H2Te}\), \(\ce{H2O}\), \(\ce{H2Se}\).
The shape assumed by biological molecules like proteins is stabilized by intermolecular forces. Review the image of the peptide below and suggest the strongest intermolecular force involved:
a. ionic bonds
b. hydrogen bonds
c. London forces
d. covalent bonds
Identify the main type (strongest) of intermolecular forces that are present in liquids of the following compounds: ionic bonds, dipole–dipole, hydrogen bonds, or dispersion forces.
a. \(\ce{NBr3}\): __________
b. \(\ce{H2O}\): __________
c. \(\ce{Cl2}\): __________
d. \(\ce{NaCl}\): __________
Which of the following compounds has the highest boiling point?
a. \(\ce{CCl4}\)
b. \(\ce{H2O}\)
c. \(\ce{NH3}\)
d. \(\ce{CO2}\)
Arrange the following intermolecular forces according to their strength from strongest (1) to weakest (3).
| Intermolecular Force | Strength of Intermolecular Force |
|---|---|
| Hydrogen bond | |
| Dispersion forces | |
| Dipole-dipole |