Chapter 6- Ionic and Molecular Compounds

Question 1

Ionic bonds

Answer 1

occur when the valence electrons of atoms of a metal are transferred to atoms of a nonmetal.

Question 2

Covalent bonds

Answer 2

form when atoms of nonmetals share valence electrons.

Question 3

Ionic and Covalent Bonds

Answer 3

Chemical bonds are formed when atoms lose, gain, or share valence electrons to acquire an octet of eight valence electrons (octet rule).

Question 4

Positive Ions: Metals Lose Electrons and form Cations

Answer 4

Sodium atoms in Group 1A (1) are neutral, with 11 electrons and 11 protons. They
•lose one electron to have the same number of valence electrons as neon and a filled energy level
•will form an ion with 10 electrons and 11 protons, and an ionic charge of 1+, Na+

Question 5

Negative Ions: Gain of Electrons to form Anions

Answer 5

Chlorine atoms in Group 7A (17) are neutral, with 17 electrons and 17 protons. They
•will gain one electron to have the same number of valence electrons as argon and a filled energy level
•form an ion with 18 electrons and 17 protons, and an ionic charge of 1−, Cl−

Question 6

Write the formula and symbol of an ion with 16 protons and 18 electrons.

Answer 6

The element with 16 protons is sulfur, with the symbol S. An ion of sulfur with 18 electrons gives sulfur a chargeof 2−. The sulfide ion is
S -2

Question 7

Consider the elements calcium and chlorine.
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 acquire an octet.
D. Write the symbol, including its ionic charge, and name of each resulting ion.

Answer 7

A. Identify each as a metal or a nonmetal.calcium = metalchlorine = nonmetal
B. State the number of valence electrons for each.Calcium in Group 2A (2) has two valence electrons.Chlorine in Group 7A (17) has seven valence electrons.
C. State the number of electrons that must be lost or gained for each to acquire an octet.Calcium will lose two electrons to acquire an octet.Chlorine will gain one electron to acquire an octet.
D. Write the symbol, including its ionic charge, and name of each resulting ion.
Ca2+ Calcium
Cl- Chloride

Question 8

Ionic Compounds

Answer 8

• consist of positive and negative ions
• have attractions called ionic bonds between positively and negatively charged ions
• have high melting points
• are solid at room temperature

Question 9

Write the ionic formula for the compound formed with Ba2+and Cl− ions.

Answer 9

Write the symbols of the ions:
Ba2+ Cl−Cancel the positive and negative charges.Cross multiply the numbers.
Writing the cation first and the anion second gives the formula BaCl2.

Question 10

Select the correct formula for each of the following ionic compounds:
A. Na+ and O2−
1. NaO 2. Na2O 3. NaO2

B. Al3+ and Cl−
1. AlCl3 2. AlCl 3. Al3Cl

C. Mg2+ and N3−
1. MgN 2. Mg2N3 3. Mg3N2

Answer 10

A. Na+ and O2−
Ans: 2. Na2O

B. Al3+ and Cl−
Ans:1. AlCl3

C. Mg2+ and N3−
Ans: 3. Mg3N2

Question 11

Naming Ionic Compounds

Answer 11

When naming an ionic compound,
•the name of the metal is written first and is the same as the name of the element
•the name of the nonmetal is the first syllable of the nonmetal name + ide ending and is written second
•a space is placed between the names of the metal and nonmetal ion

Question 12

Write the names for the following compounds:
A. CaO Fill in the blank
B.Al2S3 Fill in the blank
C.MgCl2 Fill in the blank

Answer 12

Step 4 Write the name for the cation first and the name for the anion second.
A. The name of CaO is calcium oxide.
B. The name of Al2S3 is aluminum sulfide.
C. The name of MgCl2 is magnesium chloride.

Question 13

Metals with Variable Charges

Answer 13

Transition elements except for Zn2+, Cd2+, and Ag+ form two or more positive ions (cations). We say they have variable charge.
A Roman numeral equal to the ion charge is placed in parentheses immediately after the metal name.

Question 14

Use the charge on the anion and charge balance to calculate charge on the metal ion.
MnF2

Answer 14

Therefore, the name of MnF2 is Manganese (II) fluoride.

Question 15

Naming Ionic Compounds with Variable Charge Metals

Name the ionic compound FeCl2

Answer 15

STEP 1 Determine the charge of the cation from the anion.
Fe2+

STEP 2 Name the cation by its element name and use a Roman numeral in parentheses for the charge.
Iron (II)

STEP 3 Name the anion by using the first syllable of its element name followed by ide.
chloride

STEP 4 Write the name for the cation first and the name for the anion second.
Iron(II)Chloride

Question 16

Name the following ionic compound containing a variable charge metal: MnO2

Answer 16

STEP 1 Determine the charge of the cation from the anion.

STEP 2 Name the cation by its element name and use a Roman numeral in parentheses for the charge.
Manganese (IV)

STEP 3Name the anion by using the first syllable of its element name followed by ide. oxide

STEP 3Name the anion by using the first syllable of its element name followed by ide. oxide
Manganese (IV) Oxide

Question 17

Write the formula for SnCl2

Answer 17

tin(II)chloride

Question 18

Write chemical formulas for the following compounds:
A. Nickel(II)sulfide
B. Zinc Chloride
C. Iron(III)Oxide

Answer 18

STEP 3 Write the formula, cation first, using subscripts from the charge balance.
A. NiS
B. ZnCl2
C.Fe2O3

Question 19

Polyatomic Ions

Answer 19

• are a group of atoms with an overall charge
• often consist of a nonmetal such as phosphorus, sulfur, carbon, or nitrogen covalently bonded to oxygen atoms
• usually have a 1−, 2−, or 3− charge
• have a negative charge except for NH4+, ammonium, which has a positive charge

Question 20

Writing Formulas for Compounds Containing Polyatomic Ions

Answer 20

When writing formulas for ionic compounds containing polyatomic ions, we use the same rules of charge balance as those for simple ionic compounds.
Consider the formula for magnesium nitrate:
Mg(NO3)2

Question 21

Write the formula for aluminum bicarbonate.

Answer 21

Al (HCO3)3

Question 22

Write the formula for sodium phosphate.

Answer 22

Na 3 PO 4

Question 23

Write the correct formula for each compound.
A. aluminum nitrate 
B. copper (II) nitrate 
C. iron (III) hydroxide 
D. tin (IV) hydroxide

Answer 23

A. Al(NO3)3
B. Cu(NO3)2
C. Fe(OH)3
D. Sn(OH)4

Question 24

Name the following ionic compounds:
A. Ca(NO3)2
B. SnSO4

Answer 24

A. Calcium nitrate

B. tin(II)Sulfide

Question 25

Name the following ionic compounds: A. MgSO3 B.MgSO4 C. Pb3(PO3)2

Answer 25

A. Magnesium sulfite B. Magnesium sulfite C. lead(II)Phosphite

Question 26

Molecular Compounds: Sharing Electrons Learning Goal Given the formula of a molecular compound, write its correct name; given the name of a molecular compound, write its formula.

Answer 26

The names of molecular compounds need prefixes because several different compounds can be formed from the same two nonmetals.

Question 27

When naming a molecular compound:

Answer 27

* the first nonmetal in the formula is named by its element name * the second nonmetal is named by using the first syllable of its name followed by ide When a subscript indicates two or more atoms of an element, a prefix is used in front of its name.

Question 28

Select the correct name for each molecular compound: A. SiCl4 B. P2O5 C. Cl2O7

Answer 28

A. silicon tetrachloride B. diphosphorus pentaoxide C. dichlorine heptoxide

Question 29

``` Identify each compound as ionic or molecular, and give its correct name. A. SO3 B. BaCl2 C. (NH4)3PO3 D. Cu2CO3 E. N2O4 ```

Answer 29

A. SO3 molecular, sulfur trioxide B. BaCl2 ionic, barium chloride C. (NH4)3PO3 ionic, ammonium phosphite D. Cu2CO3 ionic, copper(I) carbonate E. N2O4 molecular, dinitrogen tetroxide

Question 30

Lewis Structures for Molecules Learning Goal Draw the Lewis structures for molecular compounds with single and multiple bonds.

Answer 30

Lewis structures use Lewis symbols to diagram the sharing of valence electrons for single and multiple bonds in molecules.

Question 31

o draw the Lewis structure for a fluorine molecule, F2,

Answer 31

* we start with two fluorine atoms each with seven valence electrons * each fluorine atom shares one electron to form a covalent bond, giving each fluorine an octet

Question 32

Drawing Lewis structures

Answer 32

* To draw the Lewis structure for methane, CH4, we start by drawing the Lewis symbols for carbon and hydrogen. * Carbon needs four hydrogen atoms to complete the noble gas configurations for carbon and hydrogen.

Question 33

Draw the Lewis structure for the following- A. PF3 B. H2S C. CCl4

Answer 33

on slide 63

Question 34

Diatomic Molecules

Answer 34

The elements hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine exist as diatomic molecules. There are seven diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2.

Question 35

electronegativity

Answer 35

The electronegativity value of an element indicates the attraction of an atom for the shared electrons in a bond. Electronegativity •increases from left to right going across a period on the periodic table •increases from the bottom to the top of the periodic table •is high for the nonmetals, with fluorine as the highest •is low for the metals

Question 36

nonpolar covalent bond

Answer 36

A nonpolar covalent bond •occurs between nonmetals •is an equal or almost equal sharing of electrons by two bonding atoms •has a very small electronegativity difference examples: N-N 3.0 − 3.0 = 0.0 Nonpolar covalent

Question 37

Variations in Bonding - | electronegativity

Answer 37

The difference in electronegativity values for two atoms can be used to predict the type of chemical bond. •If the electronegativity difference is between 0 and 0.4, the bond is nonpolar covalent. •If the electronegativity difference is between 0.5 and 1.8, the bond is polar covalent. •If the electronegativity difference is between 1.9 and 3.3, the bond is ionic.

Question 38

polar covalent bond

Answer 38

``` A polar covalent bond •occurs between nonmetal atoms •is an unequal sharing of electrons •has a moderate electronegativity difference O---Cl 3.5 − 3.0 = 0.5 Polar covalent ```

Question 39

``` Use the electronegativity difference to identify the type of bond—nonpolar covalent, polar covalent, or ionic—between the following: A. K-N B. N-O C. Cl-Cl D. H-Cl ```

Answer 39

A. 2.2 Ionic B. 0.5 polar covalent C. 0.0 nonpolar covalent D. 0.9 polar covalent

Question 40

``` Use the electronegativity difference to identify the type of bond—nonpolar covalent, polar covalent, or ionic—between the following: A. K-N B. N-O C. Cl-Cl D. H-Cl ```

Answer 40

A. 2.2 Ionic B. 0.5 polar covalent C. 0.0 nonpolar covalent D. 0.9 polar covalent

Question 41

Valence shell electron-pair repulsion (VSEPR) theory

Answer 41

* describes the orientation of electron groups around the central atom * states that electron groups are arranged as far apart as possible around the central atom * states that the specific shape of a molecule is determined by the number of atoms attached to the central atom

Question 42

Polarity of Molecules and intermolecular forces

Answer 42

Covalent bonds in molecules can be polar or nonpolar. The bonds in a molecule and its shape determine whether that molecule is classified as polar or nonpolar.

Question 43

Dipoles: Nonpolar Molecules

Answer 43

Nonpolar molecules •such as H2, Cl2, and O2 are nonpolar because they contain nonpolar covalent bonds •with polar bonds can be nonpolar if the dipoles in the polar bonds cancel each other in a symmetrical arrangement such as in CO2 and CCl4

Question 44

Dipoles: Polar Molecules

Answer 44

Polar molecules such as HCl are polar because •one end of the molecule is more negatively charged than the other •the polar bonds in the molecule do not cancel each other •the electrons are shared unequally in the polar covalent bond In polar molecules such as H2O, •there are two lone pairs and two bonds around the central atom •there are dipoles that do not cancel, making the molecule positive at one end and negative at the other end •there is a partial negative charge on the central atom

Question 45

Dipole–Dipole Attractions

Answer 45

In covalent compounds, polar molecules •exert attractive forces called dipole–dipole attractions •have dipoles where the positively charged end of the dipole in one molecule is attracted to the negatively charged end of the dipole in another molecule

Question 46

Hydrogen Bonds

Answer 46

In covalent compounds, polar molecules form strong dipole attractions called hydrogen bonds between hydrogen atoms bonded to F, O, or N and a lone pair on F, O, or N. Hydrogen bonds are the strongest force between molecules and play a major role in the shape of DNA.

Question 47

Dispersion Forces

Answer 47

Dispersion forces are •weak attractions between nonpolar molecules •caused by temporary dipoles that develop when molecules bump into each other •weak but make it possible for nonpolar molecules to form liquids and solids

Question 48

Identify the main type of attractive forces that are present in liquids of the following compounds: ionic bonds, dipole–dipole, hydrogen bonds, or dispersion forces. A. NCl3 B. H2O C. Br---Br D. KCl E. NH3

Answer 48

``` A. NCl3 dipole–dipole forces B. H2O hydrogen bonds C. Br----Br dispersion forces D. KCl ionic bonds E. NH3 hydrogen bonds ```

Question 49

``` Identify the strongest attractive forces between the particles of each of the following. A.CH3Cl B. H2 C. CH3COOH D. SiH4 ```

Answer 49

A.CH3Cl = Dipole-dipole attraction B. H2 =Dispersion forces C. CH3COOH = Hydrogen bonding D. SiH4 = Dispersion forces Nonpolar molecules, in which there are little to no differences in electronegativity between the atoms, are only capable of temporary dipoles, and the resulting weak attractions between nonpolar molecules are considered dispersion forces. Permanent dipoles in polar molecules allow for stronger attractions between the partial positive charges and partial negative charges of molecules, which are referred to as dipole-dipole interactions. An even stronger type of dipole-dipole interaction can occur when the dipole involves a bond between hydrogen and fluorine, oxygen, or nitrogen, and that is referred to as a hydrogen bond.

Question 50

Which of the following elements does not exist as a diatomic molecule? ``` nitrogen chlorine carbon hydrogen oxygen ```

Answer 50

carbon

Question 51

Which one of the following molecules contains polar bonds? KBr Cl2 SO2 BH3

Answer 51

SO2

Question 52

TRue or FAlse | Chlorine is more electronegative than bromine.

Answer 52

True

Question 53

Which of the following substances contains a nonpolar covalent bond? ``` N2 NH3 MgF2 NaCl H2O ```

Answer 53

N2

Question 54

Which of the following compounds contains a polar covalent bond? ``` O2 HCl Br2 MgO NaF ```

Answer 54

HCl

Question 55

The bond in Cl2 is a(n) ________. ``` metallic bond polar ionic bond ionic bond no bond nonpolar covalent bond ```

Answer 55

nonpolar covalent bond

Question 56

Which one of the following molecules contains nonpolar bonds? carbon tetrahydride sodium chloride sulfur dichloride phosphorus trifluoride

Answer 56

carbon tetrahydride

Question 57

True or False The strongest attractive forces between molecules of NH3 are hydrogen bonds.

Answer 57

True

Question 58

Which compound describes the strongest attractive forces present in a sample of glucose (C6H12O6) to make it a solid? ionic bonds dispersion forces hydrogen bonding covalent bond

Answer 58

hydrogen bonding

Question 59

The four major attractive forces between particles are ionic bonds, dipole-dipole attractions, hydrogen bonds, and dispersion forces. Consider the compounds below, and classify each by its predominant attractive or intermolecular force among atoms or molecules of the same type. Drag each item to the appropriate bin. NaCl HCl F2 H2O

Answer 59

``` NaCl = Ionic HCl = Dipole F2 = Dispersion H2O = H bonding ```

Question 60

Li2CO3, an antidepressant | Spell out the full name of the compound.

Answer 60

lithium carbonate Ionic compounds do not require prefixes in their names because they are formed from ions with predictable charges. When reading the name of this lithium salt, you can predict the chemical formula because lithium only forms a cation with a +1 charge, and carbonate is an anion with a − 2 charge.

Question 61

MgSO4, Epsom salts | Spell out the full name of the compound.

Answer 61

magnesium sulfate

Question 62

K2CO3, a diuretic | Spell out the full name of the compound.

Answer 62

potassium carbonate

Question 63

Na3PO4, a laxative | Spell out the full name of the compound.

Answer 63

sodium phosphate All of these ionic compounds are composed of ions with one type of charge. Most transition metals, in contrast, can form different types of ions (having different charges). Therefore, their names should indicate the type of charge using Roman numerals. For example, FeO is iron(II) oxide (containing the Fe2+ ion), and Fe2O3 is iron(III) oxide (containing the Fe3+ ion).

Question 64

Ba(OH)2, a component of antacids

Answer 64

Barium hydroxide Ionic compounds do not require prefixes in their names because they are formed from ions with predictable charges. When reading the name of this barium salt, you can predict the chemical formula because barium, in group 2A (2), only forms a cation with a 2+ charge, and hydroxide is an anion with a 1 − charge.

Question 65

magnesium chloride | Express your answer as a chemical formula.

Answer 65

MgCl2 Magnesium is in group 2A (2) and forms a 2+ cation. The element chlorine is in group 7A (17) and forms a 1 − anion. Two chloride ions charge balance the magnesium ion. total charge on compound=[(1 Mg)×(2+)]+[(2 Cl)×(1−)] = 0

Question 66

sodium sulfide | Express your answer as a chemical formula.

Answer 66

Na2S The element sodium is in group 1A (1) and forms a 1+ cation. Sulfur is in group 6A (16) and forms a 2 − anion. Two sodium ions charge balance the sulfide ion. total charge on compound=[(2 Na)×(1+)]+[(1 S)×(2−)] = 0

Question 67

copper(I) oxide | Express your answer as a chemical formula.

Answer 67

Cu2O Since copper is a transition element and form ions with variable charges, the Roman numeral (I) indicates that the 1+ cation is in this compound. Oxygen is in group 6A (16) and forms a 2 − anion. total charge on compound=[(2 Cu)×(1+)]+[(1 O)×(2−)] = 0

Question 68

zinc phosphide | Express your answer as a chemical formula.

Answer 68

Zn3P2 Transition elements form more than one positive ion, except for Zn2+ , Cd2+ , and Ag+ . Compound names with these elements do not need a Roman numeral because their charge is known. Phosphorus is in group 5A (15). The zinc cation is charge balanced with the P3− ion. total charge on compound=[(3 Zn)×(2+)]+[(2 P)×(3−)] = 0

Question 69

nickel(III) nitride | Express your answer as a chemical formula.

Answer 69

NiN Since nickel is a transition element and forms ions with variable charges, the Roman numeral (III) indicates that the 3+ cation is in this compound. Nitrogen is in group 5A (15) and forms a 3 − anion. total charge on compound=[(1 Ni)×(3+)]+[(1 N)×(3−)] = 0

Question 70

cobalt(II) fluoride | Express your answer as a chemical formula.

Answer 70

CoF2 Since cobalt is a transition element and forms ions with a variable charges, the Roman numeral for 2 indicates the charge of the cation in this compound. Fluorine is in group 7A (17) and forms a 1 − anion. total charge on compound=[(1 Co)×(2+)]+[(2 F)×(1−)] = 0

Question 71

Al2(SO4)3, an antiperspirant | Spell out the full name of the compound.

Answer 71

Aluminum sulfate Aluminum sulfate is an ionic compound because an ionic bond forms between the metal cation and nonmetal anion. The ions in the compound are Al3+ and SO42− . Roman numerals are unnecessary in its name because aluminum forms only one type of cation.

Question 72

CaCO3, an antacid | Spell out the full name of the compound.

Answer 72

Calcium carbonate

Question 73

N2O, “"laughing gas," an inhaled anesthetic | Spell out the full name of the compound.

Answer 73

dinitrogen monoxide Both elements in dinitrogen monoxide are nonmetals, which signifies that a covalent bond forms between them (i.e., it is a molecular compound). Molecules usually also have common names. For example, N2O may be referred to as laughing gas or nitrous oxide, and SeO2 may be referred to as selenoyl or downeyite (a mineral). Sometimes, the common name is similar to the systematic name (like nitrous oxide), but the systematic names of molecules always employ prefixes. When there are no subscripts, the mono prefix is used for the second element (e.g., CO is carbon monoxide). Laughing gas and nitrous oxide are considered common names for N2O , but you should provide the systematic name. Recall that the names of molecular compounds require prefixes because more than one molecular compound can be formed from two nonmetal elements.

Question 74

Mg(OH)2, a laxative | Spell out the full name of the compound.

Answer 74

Magnesium hydroxide

Question 75

tin(II) sulfide | Express your answer as a chemical formula.

Answer 75

SnS

Question 76

lead(IV) oxide | Express your answer as a chemical formula.

Answer 76

PbO2

Question 77

silver chloride | Express your answer as a chemical formula.

Answer 77

AgCl

Question 78

calcium nitride | Express your answer as a chemical formula.

Answer 78

Ca3N2

Question 79

copper(I) phosphide | Express your answer as a chemical formula.

Answer 79

Cu3P

Question 80

chromium(II) bromide | Express your answer as a chemical formula.

Answer 80

CrBr2

Question 81

Enter the formula for the polyatomic ion of Na2CO3. Express your answer as an ion. Express single charges as [+], not [1+].

Answer 81

CO32− The polyatomic anion in this compound has the formula CO32− and is charge balanced by two 1+ cations

Question 82

Name Na2CO3. | Spell out the full name of the compound.

Answer 82

sodium carbonate

Question 83

Enter the formula for the polyatomic ion of (NH4)2O. | Express your answer as an ion. Express single charges as [+], not [1+].

Answer 83

NH4+ The cation in this compound is one of the few positively charged polyatomic ions and has the formula NH+4 . Two of these cations charge balance one 2 − anion.

Question 84

Name (NH4)2O. | Spell out the full name of the compound.

Answer 84

Ammonium oxide The ammonium cation is the only common polyatomic ion that is positively charged. The anion is the oxide anion, which has a 2 − charge.

Question 85

Enter the formula for the polyatomic ion of Mg(OH)2. | Express your answer as an ion. Express single charges as [+], not [1+].

Answer 85

OH- The anion in this ionic compound is OH− . Two of these polyatomic ions charge balance the cation Mg2+ .

Question 86

``` Name Mg(OH)2. Spell out the full name of the compound. ```

Answer 86

magnesium hydroxide The hydroxide ion has a 1 − charge. Since the element magnesium is in group 2A (2), it forms a 2+ ion.

Question 87

Enter the formula for the polyatomic ion of Ge(NO2)2. | Express your answer as an ion. Express single charges as [+], not [1+].

Answer 87

NO2− This nitrogen-containing polyatomic anion is NO2− . Two of these anions charge balance the cation Ge .

Question 88

``` Name Ge(NO2)2. Spell out the full name of the compound. ```

Answer 88

germanium nitrite The nitrite ion has a 1 − charge. Since two of these polyatomic ions charge balance one ion of Ge , the charge of the cation is 2+. Therefore, the Roman numeral II is needed in the name because the transition metal germanium can form variable charges.

Question 89

Enter a name for FePO3. | Spell out the full name of the compound.

Answer 89

iron(III) phosphite Fe is a transition metal and it can form ions with variable charges. Roman numerals are used in the name to show the charge of this ion. Given that PO33− has a charge of 3 − and there is one ion of PO33− , the charge of Fe must be 3+. Therefore, the name is iron(III) phosphite.

Question 90

Enter a name for Cl2O7. | Spell out the full name of the compound.

Answer 90

dichlorine heptoxide Both chlorine and oxygen are nonmetals. Therefore, this is a molecular compound. Prefixes are used in the names of molecular compounds to denote the number of atoms of each element. Since there is more than one atom of chlorine in the molecule, it does need the prefix di before the element name in the molecule name.

Question 91

Prefix for atoms

Answer 91

``` 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca ```

Question 92

Enter a name for Ca3(PO4)2. | Spell out the full name of the compound.

Answer 92

Calcium phosphate The polyatomic ion phosphate has the formula PO43− . In this ionic compound the cation calcium is named first, followed by phosphate. Since calcium is a group 2A (2) metal and has a predictable charge, no Roman numerals are required to indicate the charge on the cation.

Question 93

Enter a name for PCl3. | Spell out the full name of the compound.

Answer 93

phosphorus trichloride Both phosphorus and chlorine are nonmetals. Therefore, this is a molecular compound. Prefixes are used in the names of molecular compounds to denote the number of atoms of each element.

Question 94

Enter a name for Al(ClO)3. | Spell out the full name of the compound.

Answer 94

aluminum hypochlorite The polyatomic ion hypochlorite has the formula ClO− . This compound is ionic, because of the presence of hypochlorite and the metal cation. The cation aluminum is named first, followed by hypochlorite .

Question 95

Enter a name for Co(C2H3O2)2. | Spell out the full name of the compound.

Answer 95

cobalt(II) acetate The polyatomic ion acetate has the formula C2H3O2− . This compound is ionic, due to the presence of acetate and a metal. The cation cobalt is named first, followed by acetate. There are two ions of acetate and one ion of cobalt, so the charge on cobalt is 2+. Because cobalt can form ions with variable charges, its charge is written in Roman numerals immediately after it, in parentheses and with no spaces. The name is cobalt(II) acetate .

Question 96

Enter a name for SrCO3. | Spell out the full name of the compound.

Answer 96

strontium carbonate The polyatomic ion carbonate has the formula CO32− . This compound is ionic, because of the presence of carbonate and a metal. The cation strontium is named first, followed by carbonate.

Question 97

Classify each of the following as ionic or molecular. ``` SrCo3 Al(ClO)3 FePO3 Ca3(PO4)2 Co(C2H3O2)2 Cl2O7 PCl3 ```

Answer 97

``` SrCo3 (Ionic) Al(ClO)3 (Ionic) FePO3 (Ionic) Ca3(PO4)2 (Ionic) Co(C2H3O2)2 (Ionic) ``` Cl2O7 (molecular) PCl3 (molecular)