Ch 11/12 Flashcards

0
Q

Valence electrons

A

Electrons involved in chemical bonds

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1
Q

What is a Chemical bond

A

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

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2
Q

Ionic

A

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

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3
Q

Electro negativity of ionic bonds

A

1.7-4

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4
Q

Covalent bonds

A

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

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5
Q

Electronegativity of non polar covalent

A

0-.4

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6
Q

Electro negativity of polar covalent bonds

A

.4-1.7

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7
Q

Metallic. Bonds

A

Metal and metal
Sea of electrons
No electro negativity

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8
Q

Isoelectronic

A

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

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9
Q

Most stable number of valence electrons

A

8 or an octet

Exception of He with 2

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10
Q

Electronegativity

A

A measure of how well an atom attracts electrons

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11
Q

How do metal atoms become Isoelectronic

A

They lose electrons

Becomes positive cation

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12
Q

How do non metals become Isoelectronic

A

They gain electrons

Becomes negative anion

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13
Q

Electrostatic attraction

A

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

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14
Q

Polyatomic ions

A

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

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15
Q

Common ion charges

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

Lattice energy

A

Measure of how much energy is released when bonds form

The more energy released, the stronger the bond

17
Q

Ionic compounds

A
Form lattice crystals
Brittle
High melting points
Soluble
Form electrolytes
18
Q

Pairs of bonds

A

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

19
Q

Non polar

A

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

20
Q

Polar

A

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

21
Q

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

A

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

22
Q

4 effective pairs

A

Tetrahedral arrangement

23
Q

3 effective pairs

A

Trigonal planar

24
Q

2 effective pairs

A

Linear

25
Q

Bond energy

A

Measure of the strength of a covalent bond

26
Q

Exceptions in Lewis Structure

A

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