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Chem > Lewis Structures > Flashcards

Lewis Structures Flashcards

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1
Q

Octet rule

A

Most atoms form bonds in order to obtain 8 valence electrons
Exceptions- Hydrogen 2, boron 6

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2
Q

How to find valence electrons

A

Down columns

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3
Q

Lewis dot structure

A

A molecular model that uses symbols and bonds to show relative positions of atoms

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4
Q

Steps to determine Lewis structure (1)

A

1-predict draw location
H always end
First element listed is normally central atom

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5
Q

Steps to determine Lewis structure (2)

A

Find number of valence electrons needed and then number they have, subtract the two to find the difference

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6
Q

Steps to determine Lewis structure (3)

A

Use the difference to divide it by two which gives number of bonds

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7
Q

Steps to determine Lewis structure (4)

A

Draw in bonds and then unpaired electrons to central atom

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8
Q

Steps to determine Lewis structure (5)

A

Count number of electrons to check work, should equal number have

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9
Q

True or false, most bonds are a blend of ionic and covalent characteristics

A

True

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10
Q

How to find bond type

A

Difference in electronegativity (subtract)

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11
Q

Electronegativity difference number for polar covalent

A

1.7-.3

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12
Q

Electronegativity difference number for no polar covalent

A

0-.3

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13
Q

How to find more polar using periodic table

A

Bigger difference between the atoms means more polar

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14
Q

Non polar covalent bond

A 
Electrons Shared equally
Symmetrical electron density
Usually identical atoms 
( •    •) 
Ex CH
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15
Q

Polar covalent

A

Electronegativity are shared unequally
Asymmetrical electron density
Results in partial charges dipoles
( • Bigger •) neg

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16
Q

What is the molecular geometry of covalent molecules is based on

A

Valence shell electron pair repulsion theory

VSEPR

17
Q

What results in the specific molecular shape and bond angles

A

Electron pairs arrange themselves to be as far as possible

18
Q

Difference between unshared electrons and shared pairs space

A

Lone pairs take up more space then shared pairs

19
Q

2 atoms to central, no lone pairs
Shape?
Bond angle?
Example?

A

Linear
180
Straight line

20
Q

3 atoms to central, 0 lone pairs
Shape?
Bond angle?
Example?

A

Triangular planar
120
O
O -S-O

21
Q

4 atoms to central, no lone pairs
Shape?
Bond angle?
Example?

A 
Tetrahedral 
109.5
    H
H-C-H
    H
22
Q

3 atoms to central, 1 lone pairs
Shape?
Bond angle?
Example?

A 
Trigonometry pyramidal 
107
     H
H-N-H
     :
23
Q

2 atoms to central, 2 lone pairs
Shape?
Bond angle?
Example?

A

Bent
104.5
Cl-S::
Cl

24
Q

When is it polar

A

When no symmetrical (lone pairs or different atoms)

Or uneven sharing of electron pairs due to large difference in electronegativity between two atoms in the bond

25
Q

IMF stands for

A

Intermolecular forces

Attractive forces between two molecules of the same compound

26
Q

What does polarity depend on

A

Attraction

27
Q

Which is stronger, polarity or chemical bonds

A

Chemical bonds

28
Q

What IMF force do all molecules have

A

London dispersion

29
Q

List weakest to strongest of imf forces

A 
Weakest-London dispersion
Dipole dipole
Hydrogen bonding (Fstrongest)
30
Q

London dispersion force

A

Attraction between two instantaneous dipoles
Asymmetrical electron distribution
All atoms

31
Q

London dispersion diagram

A

Two separate oval molecules

32
Q

For London dispersion how to tell a tie

A

Higher molar mass is a stronger IMF

33
Q

Dipole dipole definition

A

Attraction between two permanent dipoles

Polar

34
Q

Diagram for dipole dipole

A

Hydrogen bonded to carbon

35
Q

How to tell a tie from dipole dipole

A

Greater difference in electronegativity means stronger IMF

36
Q

Hydrogen bonding definition

A

Attraction between H-FON
Polar very strong
Not Chem bond

37
Q

How to break a tie for Hydrogen bond

A

Increase in lone pairs in crease in IMF

FON order, F strongest IMF

38
Q

IMF with phase change

Weaker when

A

Boiling point is lower
Melting point lower
Evaporation faster

39
Q

IMF with phase change is stronger when

A

Boiling point higher
Melting point high
Evaporation slower

Chem (14 decks)

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