Ch 11/12

Question 0

Valence electrons

Answer 0

Electrons involved in chemical bonds

Question 1

What is a Chemical bond

Answer 1

The force of attraction that holds atoms or ions together in a chemical substance

Question 2

Ionic

Answer 2

Metal and nonmetal
Formed when Electrons are transferred due to differences in electronegativity and ionization energy
Commonly called salts

Question 3

Electro negativity of ionic bonds

Answer 3

1.7-4

Question 4

Covalent bonds

Answer 4

Non metal and non metal
Electrons are shared equally
Commonly called molecules

Question 5

Electronegativity of non polar covalent

Answer 5

0-.4

Question 6

Electro negativity of polar covalent bonds

Answer 6

.4-1.7

Question 7

Metallic. Bonds

Answer 7

Metal and metal
Sea of electrons
No electro negativity

Question 8

Isoelectronic

Answer 8

When an atom gains or loses electrons to have the same number of electrons as the nearest noble gas

Question 9

Most stable number of valence electrons

Answer 9

8 or an octet

Exception of He with 2

Question 10

Electronegativity

Answer 10

A measure of how well an atom attracts electrons

Question 11

How do metal atoms become Isoelectronic

Answer 11

They lose electrons

Becomes positive cation

Question 12

How do non metals become Isoelectronic

Answer 12

They gain electrons

Becomes negative anion

Question 13

Electrostatic attraction

Answer 13

The attraction between oppositely charged ions that makes atoms stick together in an ionic bond

Question 14

Polyatomic ions

Answer 14

Groups of atoms that have an overall charge and act like a single ion

Question 15

Common ion charges

Answer 15

Group 1- loses 1
Group 2- loses 2
Group 13- loses 3
Group 15- gains 3
Group 16- gains 2
Group 17- gains 1

Question 16

Lattice energy

Answer 16

Measure of how much energy is released when bonds form

The more energy released, the stronger the bond

Question 17

Ionic compounds

Answer 17

Form lattice crystals
Brittle
High melting points
Soluble
Form electrolytes

Question 18

Pairs of bonds

Answer 18

One pair- single bond
2 pairs- double bond
3 pairs- triple bond

Question 19

Non polar

Answer 19

When EN is less than .4 so neither electron can win so they share the atoms equally

Question 20

Polar

Answer 20

When the EN is greater than .4 and one atom pulls the electrons closer to itself, making it partially negative and one atom becomes positive

Question 21

How to tell which side is positive and which side is negative

Answer 21

The atom with the greater EN is the negative side of the molecule

Question 22

4 effective pairs

Answer 22

Tetrahedral arrangement

Question 23

3 effective pairs

Answer 23

Trigonal planar

Question 24

2 effective pairs

Answer 24

Linear

Question 25

Bond energy

Answer 25

Measure of the strength of a covalent bond

Question 26

Exceptions in Lewis Structure

Answer 26

Hydrogen never in middle and only has two electrons(one line) Carbon always in middle Closest element to fluorine in middle Boron only needs six electrons