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BioChemistry - Chem 109 @Ohlone > Chapter 6- Ionic and Molecular Compounds > Flashcards

Chapter 6- Ionic and Molecular Compounds Flashcards

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1
Q

Ionic bonds

A

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

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2
Q

Covalent bonds

A

form when atoms of nonmetals share valence electrons.

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3
Q

Ionic and Covalent Bonds

A

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

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4
Q

Positive Ions: Metals Lose Electrons and form Cations

A

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+

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5
Q

Negative Ions: Gain of Electrons to form Anions

A

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−

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6
Q

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

A

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

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7
Q

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.

A

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

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8
Q

Ionic Compounds

A
  • 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
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9
Q

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

A

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.

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10
Q

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

A

A. Na+ and O2−
Ans: 2. Na2O

B. Al3+ and Cl−
Ans:1. AlCl3

C. Mg2+ and N3−
Ans: 3. Mg3N2

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11
Q

Naming Ionic Compounds

A

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

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12
Q

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

A

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.

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13
Q

Metals with Variable Charges

A

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.

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14
Q

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

A

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

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15
Q

Naming Ionic Compounds with Variable Charge Metals

Name the ionic compound FeCl2

A

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

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16
Q

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

A

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

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17
Q

Write the formula for SnCl2

A

tin(II)chloride

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18
Q

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

A

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

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19
Q

Polyatomic Ions

A
  • 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
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20
Q

Writing Formulas for Compounds Containing Polyatomic Ions

A

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

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21
Q

Write the formula for aluminum bicarbonate.

A

Al (HCO3)3

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22
Q

Write the formula for sodium phosphate.

A

Na 3 PO 4

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23
Q 
Write the correct formula for each compound.
A. aluminum nitrate 
B. copper (II) nitrate 
C. iron (III) hydroxide 
D. tin (IV) hydroxide
A

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

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24
Q

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

A

A. Calcium nitrate

B. tin(II)Sulfide

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25
Q

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

A

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

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26
Q

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.

A

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

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27
Q

When naming a molecular compound:

A
  • 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.

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28
Q

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

A

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

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29
Q 
Identify each compound as ionic or molecular, and give its correct name.
A. SO3
B. BaCl2
C. (NH4)3PO3
D. Cu2CO3
E. N2O4
A

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

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30
Q

Lewis Structures for Molecules

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

A

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

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31
Q

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

A
  • 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
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32
Q

Drawing Lewis structures

A
  • 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.
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33
Q

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

A

on slide 63

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34
Q

Diatomic Molecules

A

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.

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35
Q

electronegativity

A

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

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36
Q

nonpolar covalent bond

A

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

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37
Q

Variations in Bonding -

electronegativity

A

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.

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38
Q

polar covalent bond

A 
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
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39
Q 
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
A

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

40
Q 
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
A

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

41
Q

Valence shell electron-pair repulsion (VSEPR) theory

A
  • 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
42
Q

Polarity of Molecules and intermolecular forces

A

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.

43
Q

Dipoles: Nonpolar Molecules

A

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

44
Q

Dipoles: Polar Molecules

A

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

45
Q

Dipole–Dipole Attractions

A

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

46
Q

Hydrogen Bonds

A

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.

47
Q

Dispersion Forces

A

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

48
Q

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

A 
A. NCl3      dipole–dipole forces
B. H2O       hydrogen bonds
C. Br----Br    dispersion forces
D. KCl         ionic bonds
E. NH3        hydrogen bonds
49
Q 
Identify the strongest attractive forces between the particles of each of the following.
A.CH3Cl
B. H2
C. CH3COOH
D.  SiH4
A

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.

50
Q

Which of the following elements does not exist as a diatomic molecule?

nitrogen
chlorine
carbon
hydrogen
oxygen
A

carbon

51
Q

Which one of the following molecules contains polar bonds?

KBr
Cl2
SO2
BH3

A

SO2

52
Q

TRue or FAlse

Chlorine is more electronegative than bromine.

A

True

53
Q

Which of the following substances contains a nonpolar covalent bond?

N2
NH3
MgF2
NaCl
H2O
A

N2

54
Q

Which of the following compounds contains a polar covalent bond?

O2
HCl
Br2
MgO
NaF
A

HCl

55
Q

The bond in Cl2 is a(n) ________.

metallic bond
polar ionic bond
ionic bond
no bond
nonpolar covalent bond
A

nonpolar covalent bond

56
Q

Which one of the following molecules contains nonpolar bonds?

carbon tetrahydride
sodium chloride
sulfur dichloride
phosphorus trifluoride

A

carbon tetrahydride

57
Q

True or False

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

A

True

58
Q

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

A

hydrogen bonding

59
Q

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

A 
NaCl = Ionic
HCl  = Dipole
F2   = Dispersion
H2O =  H bonding
60
Q

Li2CO3, an antidepressant

Spell out the full name of the compound.

A

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.

61
Q

MgSO4, Epsom salts

Spell out the full name of the compound.

A

magnesium sulfate

62
Q

K2CO3, a diuretic

Spell out the full name of the compound.

A

potassium carbonate

63
Q

Na3PO4, a laxative

Spell out the full name of the compound.

A

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).

64
Q

Ba(OH)2, a component of antacids

A

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.

65
Q

magnesium chloride

Express your answer as a chemical formula.

A

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

66
Q

sodium sulfide

Express your answer as a chemical formula.

A

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

67
Q

copper(I) oxide

Express your answer as a chemical formula.

A

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

68
Q

zinc phosphide

Express your answer as a chemical formula.

A

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

69
Q

nickel(III) nitride

Express your answer as a chemical formula.

A

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

70
Q

cobalt(II) fluoride

Express your answer as a chemical formula.

A

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

71
Q

Al2(SO4)3, an antiperspirant

Spell out the full name of the compound.

A

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.

72
Q

CaCO3, an antacid

Spell out the full name of the compound.

A

Calcium carbonate

73
Q

N2O, “”laughing gas,” an inhaled anesthetic

Spell out the full name of the compound.

A

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.

74
Q

Mg(OH)2, a laxative

Spell out the full name of the compound.

A

Magnesium hydroxide

75
Q

tin(II) sulfide

Express your answer as a chemical formula.

A

SnS

76
Q

lead(IV) oxide

Express your answer as a chemical formula.

A

PbO2

77
Q

silver chloride

Express your answer as a chemical formula.

A

AgCl

78
Q

calcium nitride

Express your answer as a chemical formula.

A

Ca3N2

79
Q

copper(I) phosphide

Express your answer as a chemical formula.

A

Cu3P

80
Q

chromium(II) bromide

Express your answer as a chemical formula.

A

CrBr2

81
Q

Enter the formula for the polyatomic ion of Na2CO3.

Express your answer as an ion. Express single charges as [+], not [1+].

A

CO32−

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

82
Q

Name Na2CO3.

Spell out the full name of the compound.

A

sodium carbonate

83
Q

Enter the formula for the polyatomic ion of (NH4)2O.

Express your answer as an ion. Express single charges as [+], not [1+].

A

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.

84
Q

Name (NH4)2O.

Spell out the full name of the compound.

A

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.

85
Q

Enter the formula for the polyatomic ion of Mg(OH)2.

Express your answer as an ion. Express single charges as [+], not [1+].

A

OH-

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

86
Q 
Name Mg(OH)2.
Spell out the full name of the compound.
A

magnesium hydroxide

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

87
Q

Enter the formula for the polyatomic ion of Ge(NO2)2.

Express your answer as an ion. Express single charges as [+], not [1+].

A

NO2−

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

88
Q 
Name Ge(NO2)2.
Spell out the full name of the compound.
A

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.

89
Q

Enter a name for FePO3.

Spell out the full name of the compound.

A

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.

90
Q

Enter a name for Cl2O7.

Spell out the full name of the compound.

A

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.

91
Q

Prefix for atoms

A 
1	mono
2	di
3	tri
4	tetra
5	penta
6	hexa
7	hepta
8	octa
9	nona
10	deca
92
Q

Enter a name for Ca3(PO4)2.

Spell out the full name of the compound.

A

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.

93
Q

Enter a name for PCl3.

Spell out the full name of the compound.

A

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.

94
Q

Enter a name for Al(ClO)3.

Spell out the full name of the compound.

A

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 .

95
Q

Enter a name for Co(C2H3O2)2.

Spell out the full name of the compound.

A

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 .

96
Q

Enter a name for SrCO3.

Spell out the full name of the compound.

A

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.

97
Q

Classify each of the following as ionic or molecular.

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

Cl2O7 (molecular)
PCl3 (molecular)

BioChemistry - Chem 109 @Ohlone (5 decks)

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