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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
Q

Electronegativity

A

Measure of how well atoms are attracted to shared electrons

26
Q

What happens when electronegativity increases

A

Size decreases

27
Q

What has the highest EN

A

F

28
Q

What has the lowest EN

A

Fr

29
Q

Non polar covalent bond

A

When atoms are equal 0

30
Q

Slight polar covalent bond

A

0.1-0.5

31
Q

Polar covalent bond

A

0.6-1.6

32
Q

Ionic bond

A

1.7 and above

33
Q

Ionic crystals

A

Form crystal lattices due to bond from anions and cattions

34
Q

Formula unit

A

Shows smallest ratio of each ion in crystal form

35
Q

Molecular structures

A

Covalent bonds

36
Q

Stereochemisty

A

The study of 3D shapes and how its structure affects physical and chemical properties

37
Q

VSEPR

A

Prediction of 3D shapes

38
Q

What does VSEPR stand for

A

Valence shell electron pair repulsion

39
Q

What are rules for predicting shape

A

Electron pairs are far away
Multiple bonds are treated as one

40
Q

What does A stand for

A

Central atom

41
Q

What does X stand for

A

Bonding pair

42
Q

What does E stand for

A

Lone pair

43
Q

Linear

A

All bonding pairs and flat

44
Q

Trigonal Planar

A

All bonding pairs

45
Q

Tetrahedral

A

All bonding pairs

46
Q

Trigonal pyramidal

A

3 bonding pairs and one lone pair

47
Q

Bent

A

2 bonding pairs and 2 lone pairs

48
Q

Dipole arrow

A

Represents which has more EN

49
Q

What are each of the VSEPR shapes

A

Linear
Bent
Trigonal Planar
Trigonal Pyramidal
Tetrahedral

50
Q

Intra molecular forces

A

Forces involved within same molecule

51
Q

Intermolecular forces

A

Forces between molecules

52
Q

Strongest bond

A

Ionic bonds

53
Q

Hydrogen bonds

A

Helps bond molecules two different

54
Q

FON

A

Flouride
Oxygen
Nitrogen

55
Q

Dipole Dipole forces

A

Occours between polar molecules that dont have hydrogen bonds

56
Q

London dispersion forces

A

Only force acting on non polar molecules

57
Q

London dispersion forces 2

A

On all molecules but on non polar

58
Q

Are linear or branches stronger

A

Linear

59
Q

Why is a London dispersion force so strong

A

Since it has cattions and anaions attacted

60
Q

What causes the strongest LD force

A

The bigger and most electrons

61
Q
A

Chem 20-1 Unit 1 (5 decks)

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