Chemical Bonds I

Question 1

Chemical Bonds

Answer 1

1. Attraction between atoms or ions

2. Are due to the attraction between the positive nucleus and the negative electrons

Question 2

Potential Energy

Answer 2

Stored in bonds between atoms/ions

Question 3

Chemical Energy

Answer 3

Energy involved in making/breaking bonds

Question 4

Energy Changes in Bonds

Answer 4

1. When two atoms are bonded –> lower/stable potential energy level
2. When stronger bonds form –> Exothermic Reaction + Less potential energy

Question 5

Relationship between stabiltilty and potential energy

Answer 5

Inverse

Question 6

Exothermic vs Endothermic

Answer 6

Exothermic: Stability is high, potential energy is low when compared to reactants
Endothermic: Stability is low, potential energy is high when compared to reactants

Question 7

Endothermic/Exothermic Diagram

Answer 7

Bottom is potential energy

Top is kinetic energy

Question 8

Electronegativity

Answer 8

0-.3 –> NPC
.3-1.7 exclusive –> PC
>1.7 inclusive –> I

Question 9

Ionic Bonds

Answer 9

Attraction between ions

Nonmetal and Metal

Question 10

Lewis Structures for Ionic Bonds

Answer 10

Must have charges

May draw arrows, or have nonmetal have a full shell

Question 11

Properties of Ionic Compounds

Answer 11

As solids don't conduct electricity
When melted/in aqueous solution conduct electricity
High melting points
Have crystalline lattice structure
Very strong

Question 12

Covalant Bonds

Answer 12

Either equally/unequally shared electrons

Question 13

NPC

Answer 13

Shared equally between two nonmetals

END is

Question 14

PC

Answer 14

Shared unequally between two nonmetallic atoms

.3

Question 15

Properties of Covalant Compounds

Answer 15

Low melting Point
Dull
Brittle
Nonconductive

Question 16

Network Solid

Answer 16

Chemical compound where the atoms are bonded covalently in a continuous network
Entire network is considered a molecule

Question 17

Properties of Network Solids

Answer 17

Very high melting point
Very strong covalent bonds
Very hard
Not soluble in water

Question 18

Examples of Network Solids

Answer 18

Diamond –> C
Silicon Dioxide –> Si02
Graphite –> C in two dimensional layers

Question 19

Coordinate Covalent Bonds

Answer 19

When both electrons from a bond are shared by only one of the two atoms

Question 20

Metallic Bonds

Answer 20

Electrons in solid metals are free travel atom to atom
Metals became cations due to loss of electrons
Attraction between the mobile electrons and the metals cause a strong bond to form
Called Sea of Electrons

Question 21

Properties of Metallic bonds

Answer 21

Luster
Ductile
Malleable
Conductor

Question 22

Localized Electron Model

Answer 22

Electron Pairs are assumed to be localized on a particular atom or in the space between two atoms.
Description of valence electron arrangement (Lewis Structure)
VSEPR
Description of atomic orbital types used to share electrons or hold lone pairs

Question 23

Lone Pair Electrons

Answer 23

Electrons located on an atom

Question 24

Bonding Electrons

Answer 24

Electrons found in the space between the atoms

Question 25

2nd Row Elements

Answer 25

C,N,O,F use octet rule | Often have fewer than eight electrons, they are very reactive

Question 26

3rd Row and heavier elements

Answer 26

Can exceed the octet rule, using empty d valence orbitals

Question 27

VSEPR

Answer 27

Valence Shell Electron Pair Repulsion

Question 28

Intramolecular

Answer 28

Involved in bringing atoms together to a compound Ionic Polar Covalent Nonpolar Covalent

Question 29

Intermolecular

Answer 29

Involved in bringing molecules together Dipole-Dipole - Strong, Unequal/Partial charges Hydrogen Bonds (H to F,O,N) - Strongest Weak/Van Dar Waal's - Weakest

Question 30

Weak Intermolecular Forces

Answer 30

Small nonpolar molecules, best in liquid/solid phases with low temp and high pressure Stronger when closer together Smaller the molecule --> weak Larger the molecule --> strong Smaller nonpolar molecules, tend to be gases at room temperature, give them low boiling points --> Noble Gasses Larger nonpolar molecules, tend to be liquids and solids at room temperature Diatomic Molecules are also examples