1. Ionic, Metallic and Covalent Bonding
Writing and Naming Formulas

2. Chemical bond
force that holds two atoms together
opposites attract

3. Chemical bonds are formed by:
the attraction between the positive nucleus of one atom and the negative electrons of another atom
or by the attraction between positive and negative ions

4. Krypton
Potassium
in water
Iron in oxygen

5. Valence electrons
electrons available to be lost, gained, or shared in the formation of chemical compounds
found in outermost energy level

6. oct –

7. Octet Rule
Atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons; stable noble gas configuration.

8. Three types of bonds:
Ionic
transfer of electrons between
metal and nonmetal (or
polyatomic ion)
2. Metallic
electron sea model;
atoms of same metal
3. Covalent –
sharing of electrons between
nonmetals; may be same or
different elements

9. atom, or a bonded group of
Ion
atom, or a bonded group of
atoms, that has a positive or
negative charge
Ionic bond
electrostatic force that holds oppositely charged particles together

11. Positive ion formation
atom loses one or more valence electrons
cations

12. Write an electron configuration for sodium.
Write an electron configuration for neon.
What is the only difference in the electron configurations of these two elements?

14. Metals tend to lose electrons to form positive ions called cations.
Metals lose all valence electrons so that next energy level is full.

15. Write an electron dot notation for each metal:
Magnesium
Aluminum
Lithium
Barium
Potassium
Gallium

16. Predict if each would lose or gain electrons when forming compounds:
Magnesium
Aluminum
Lithium
Barium
Potassium
Gallium

17. How many electrons would each lose?
Magnesium
Aluminum
Lithium
Barium
Potassium
Gallium

18. What cations would the following elements form? Write symbol and charge.
Magnesium
Aluminum
Lithium
Barium
Potassium
Gallium

19. Use group number to predict charge of metal ion for representative elements only.

20. Transition metals
d block; filling inner energy levels
most form more than one common ion
sometimes inner electrons take part in bonding

21. Transition metals that form only one common ion:
silver Ag+
zinc Zn2+

22. Negative ion formation
atom gains one or more valence electrons
anion

23. Write an electron configuration for chlorine.
Write an electron configuration for argon.
What is the only difference in the electron configurations of these two elements?

24. Nonmetals tend to gain electrons to form negative ions called
anions.
Nonmetals gain enough electrons to obtain full octet (8).

25. Write an electron dot notation for each nonmetal:
Sulfur
Nitrogen
Iodine
Phosphorus
Fluorine
Oxygen

26. Predict if each would lose or gain electrons when forming compounds:
Sulfur
Nitrogen
Iodine
Phosphorus
Fluorine
Oxygen

27. How many electrons would each gain?
Sulfur
Nitrogen
Iodine
Phosphorus
Fluorine
Oxygen

28. What anions would the following elements form?
Write symbol and charge.
Sulfur
Nitrogen
Iodine
Phosphorus
Fluorine
Oxygen

29. Use group number to predict charge on nonmetals.

30. Writing formulas for binary
ionic compounds:
Write symbol and charge for
cation and anion.
Ex: lithium and oxygen
2. Use subscripts to show
the ratio of ions.

31. Cation always written first.
Ionic formulas, subscripts show simplest ratio.

32. Write formulas for the
binary ionic compounds
formed between the
following elements:
potassium and iodine
b. magnesium and chlorine
c. sodium and sulfur
d. aluminum and nitrogen
e. aluminum and sulfur

33. Naming binary ionic compounds:
cation (metal)
name of element;
always written first
anion (nonmetal)
name of element with
an ‘ide’ ending

34. Name the binary ionic
compounds indicated by
the following formulas:
AgCl
ZnO
CaBr2
SrF2
BaO
CaCl2

35. Some metals form more than one common ion; most of the transition metals and tin and lead.

36. How form multiple ions?
Transition metals – d electrons can take part in bonding
Write noble gas notation for tin:
[Kr] 5s24d105p2
Sn2+ or Sn4+

37. The charge on the metal is written as a Roman numeral in the name of compound.
Fe2+ Cl-
FeCl2
iron(II) chloride
Fe3+ Cl-
FeCl3
iron(III) chloride

38. Transition metals that form only one common ion:
silver Ag+
zinc Zn2+

39. Metals that form only one common ion do not need Roman numeral.
NaBr sodium bromide

40. Write the formula and name
for the compounds formed
between the following ions
(use Roman numerals):
Cu2+ and Br -
Fe2+ and O2-
Pb2+ and Cl-
Hg2+ and S2-
Sn2+ and F-
Fe3+ and O2-

41. Writing names with Roman
numerals:
Determine total negative
charge.
2. Total negative charge equals
total positive charge.
Charge on one positive ion is
Roman numeral.

42. Ionic compounds containing
polyatomic ions:
Write formulas as you would
for binary ionic compounds;
use parentheses if adding
subscript to polyatomic ion.

43. Write formulas for the following compounds:
magnesium carbonate
magnesium hydroxide

44. Write formulas for the
following ionic compounds:
lithium nitrate
copper(II) sulfate
sodium carbonate
calcium nitrite
potassium perchlorate

45. When naming compounds,
do not change name of
polyatomic ion.

46. Three types of bonds:
Ionic
transfer of electrons between
metal and nonmetal (or
polyatomic ion)
2. Metallic
electron sea model;
atoms of same metal
3. Covalent –
sharing of electrons between
nonmetals; may be same or
different elements

47. Why do atoms bond?
to obtain a full outer energy level; complete octet
to become more stable; lower potential energy

48. Electronegativity (EN)
indicates relative ability of an atom to attract electrons in a chemical bond

49. Metals
low EN; tend to give up electrons
Nonmetals
high EN; tend to gain electrons

50. What happens when two nonmetals, with similar EN, react?

51. Covalent bond
chemical bond that results from the sharing of valence electrons
generally formed between two nonmetals (same or different element)
electrons are attracted by the nuclei of two different atoms

54. Molecule
formed when two or more atoms bond covalently

56. Naming binary molecular compounds
First element; use entire
element name.
2. Second element ends in –ide.
Prefixes are used to indicate
the number of atoms of each
element – the subscripts.

58. N2O4
dinitrogen tetroxide
If first element has one atom, mono omitted. CO
carbon monoxide

59. Name the following
molecular compounds:
PF3
XeF4
As2O5
CCl4

60. Write formulas for the
following compounds:
carbon dioxide
dinitrogen pentoxide
silicon tetrafluoride

61. Ionic compounds
composed of large
numbers of cations and
anions; crystal lattice
formula unit – smallest
whole number ratio of
ions

63. Molecular compounds
composed of discrete
(individual) molecules
of covalently bonded
atoms
molecular formulas do not need to be lowest ratio of atoms

64. C2H4

65. Acid
a substance that produces
hydrogen ions (H+) when
dissolved in water
molecular compound that reacts with water to form ions

67. binary acid – two elements;
hydrogen and a nonmetal
name begins with prefix
‘hydro’ and ends with ‘ic’
hydrochloric acid
HCl

68. oxyacid – hydrogen, oxygen,
and a nonmetal; many formed
from polyatomic ions
if name of polyatomic ion ends
with ‘ate’ , name of acid ends
with ‘ic’
H2SO4
sulfuric acid

69. Binary acid
hydro _____ ic acid
Oxyacid
______ ic acid

70. Name the following acids:
H2CO3
HBr

71. Writing formulas for acids:
start with H+
determine charge on nonmetal ion or polyatomic ion
add subscripts if needed
to make neutral compound

72. Write formulas for the following acids:
hydrofluoric acid
phosphoric acid

73. Electronegativity (EN)
indicates the relative ability of an atom to attract electrons in a chemical bond
Type of bond formed between two atoms depends on the difference in electronegativities (DEN) of the atoms.

75. Difference in electronegativity (DEN)
locate elements on periodic table
subtract values for EN
DEN always positive

76. Ex: hydrogen and chlorine
DEN = 3.16 – 2.20 = 0.96

77. Covalent bonds may be:
Polar covalent bond
unequal sharing of electrons
one atom pulling electrons towards itself
atom with higher EN value has a partial negative charge (d-)
atom with lower EN value has a partial positive charge (d+)

78. Ex: hydrogen and chlorine
DEN = 3.16 – 2.20 = 0.96

79. Covalent bonds may be:
Nonpolar covalent bond
electrons shared equally
no partial charges

80. Most bonds are not completely ionic or covalent.

81. DEN
Bond
Character
> 1.7
Ionic
0.4 – 1.7
polar covalent
< 0.4
nonpolar covalent

82. Classify the following bonds as nonpolar- covalent, polar-covalent, or ionic. If bond is polar-covalent, assign partial charges.
C and H
H and Br
Cs and S

83. Properties of Compounds
depend on the strength of
the attractive forces
between particles

84. Properties of ionic compounds
ions arranged in a regular repeating pattern called crystal lattice
ions held together by strong
ionic bonds

85. Properties of ionic compounds
high melting and boiling points; much energy needed to separate ions
hard, rigid, brittle solids

87. Properties of ionic compounds
do not conduct electricity in solid state

88. aqueous solutions and liquid states are electrolytes - conduct electricity since
ions are free to move

89. Properties of molecular
compounds
covalent bonds between atoms are strong, but attraction forces between molecules are weak

90. Intermolecular forces
relatively weak forces of attraction between molecules
also known as
van der Waals forces

91. Properties of molecular compounds
relatively low melting and boiling points; many gases or liquids at room temperature

92. Properties of molecular compounds
do not conduct electricity when dissolved in water; except for acids

93. Metallic bond
outer energy levels of metal atoms overlap
valence electrons are shared by several atoms; delocalized (free to move)
electron sea model

94. Metallic bond
attraction of a metallic cation for delocalized electrons

95. Properties of metals

96. Properties of metals
moderately high melting points and high boiling points; most solids are room temperature
the more delocalized electrons a metal has, the greater its strength and hardness; groups 1 & 2 soft

97. Metals are malleable (hammered into thin sheets) and ductile (drawn into wires.)

98. good conductors of heat and electricity; electrons mobile
delocalized electrons interact with light, giving metals luster (shiny)

99. Three types of bonds:
Ionic – transfer of e-
metal and nonmetal

100. 2. Metallic
electron sea model;
atoms of same metal

101. 3. Covalent – sharing of e-
nonmetals

102. Nonpolar Covalent - no charges
Polar Covalent - partial charges + -

103. James
Bond