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Chem 20-1 Unit 1 > Unit Test Review > Flashcards

Unit Test Review Flashcards

1
Q

Metals x non metals

A

Solids and ionic

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2
Q

What metal is not a solid

A

Mercury

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3
Q

What state are covalent bonds in

A

All

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4
Q

Ionic bonds

A

Metals and non metals

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5
Q

Covalent bonds

A

Metals x non metals

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6
Q

Bohr models

A

Show all of the shells

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7
Q

Lewis dot diagrams

A

Show only valence electrons

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8
Q

Octet rule

A

Make sure valence electrons are full

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9
Q

Octet rule

A

Atoms gain/ loose to fill valence shells

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10
Q

What is an exception to the octet rule

A

First energy shell has only two electron

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11
Q

Electron dot diagrams

A

Determine valence electrons
Work clockwise
Place 1 on each side and pair when there are more than 4 electrons

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12
Q

What happens to unpaired electrons

A

Are taken into ionic compounds or shared in molecular bonds

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13
Q

Ionic bonds

A

Metals lose electrons to become ions and non metals gain

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14
Q

Covalent bonds

A

Share electrons to complete valence electrons
Non metals

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15
Q

What diagram should be drawn when drawing ionic and covalent bonds

A

LDD

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16
Q

The process for drawing covalent bonds

A

Count total of valence
Atom with highest bonding e is central atom
Distriubte central then others with e making sure all have an octet

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17
Q

Lone pair

A

Are two electrons drawn beside eachother

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18
Q

Bonding electrons

A

Are electrons drawn without a pair

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19
Q

Structural formula

A

Use lines to represent bonds

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20
Q

Acid

A

Has an H in it

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21
Q

What are two exceptions to the octet rule

A

Boron has three electrons and fills at 6
Berylium has two electrons and fills at 4

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22
Q

Resonance structures

A

Is that there is more than one lewis dot diagram for a compound

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23
Q

Coordinate covalent bonds

A

When an atom gives up both electrons to form a bond

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24
Q

Metallic bonding

A

When all the metals share all the e
Make metals good conductors

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25
Electronegativity
Measure of how well atoms are attracted to shared electrons
26
What happens when electronegativity increases
Size decreases
27
What has the highest EN
F
28
What has the lowest EN
Fr
29
Non polar covalent bond
When atoms are equal 0
30
Slight polar covalent bond
0.1-0.5
31
Polar covalent bond
0.6-1.6
32
Ionic bond
1.7 and above
33
Ionic crystals
Form crystal lattices due to bond from anions and cattions
34
Formula unit
Shows smallest ratio of each ion in crystal form
35
Molecular structures
Covalent bonds
36
Stereochemisty
The study of 3D shapes and how its structure affects physical and chemical properties
37
VSEPR
Prediction of 3D shapes
38
What does VSEPR stand for
Valence shell electron pair repulsion
39
What are rules for predicting shape
Electron pairs are far away Multiple bonds are treated as one
40
What does A stand for
Central atom
41
What does X stand for
Bonding pair
42
What does E stand for
Lone pair
43
Linear
All bonding pairs and flat
44
Trigonal Planar
All bonding pairs
45
Tetrahedral
All bonding pairs
46
Trigonal pyramidal
3 bonding pairs and one lone pair
47
Bent
2 bonding pairs and 2 lone pairs
48
Dipole arrow
Represents which has more EN
49
What are each of the VSEPR shapes
Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral
50
Intra molecular forces
Forces involved within same molecule
51
Intermolecular forces
Forces between molecules
52
Strongest bond
Ionic bonds
53
Hydrogen bonds
Helps bond molecules two different
54
FON
Flouride Oxygen Nitrogen
55
Dipole Dipole forces
Occours between polar molecules that dont have hydrogen bonds
56
London dispersion forces
Only force acting on non polar molecules
57
London dispersion forces 2
On all molecules but on non polar
58
Are linear or branches stronger
Linear
59
Why is a London dispersion force so strong
Since it has cattions and anaions attacted
60
What causes the strongest LD force
The bigger and most electrons
61

Chem 20-1 Unit 1 (5 decks)

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