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physical chem > bonding (3) > Flashcards

bonding (3) Flashcards

1
Q

what is electronegativity?

A

power of an atom to attract the two electrons in a covalent bond

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2
Q

3 factors that effect electronegativity?

A

nuclear charge, atomic radius, shielding.

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3
Q

how does nuclear charge effect electronegativity?

A

more protons, stronger attraction between nucleus and bonding pair of electrons

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4
Q

how does atomic radius effect electronegativity?

A

closer to the nucleus, stronger attraction between nucleus and bonding pair of electrons

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5
Q

how does shielding effect electronegativity?

A

less shells of electrons between the nucleus and the electrons means less shielding, stronger attraction between nucleus and bonding pair of electrons

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6
Q

trend in electronegativity when going down a group

A

decreases
- atomic radius increases

-more shielding and less attraction between nucleus and bonding pair of electrons

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7
Q

trend in electronegativity across a period

A

increases since

-atomic radius decreases

-nuclear charge increases

-same shielding

therefore stronger attraction between nucleus and bonding pair of electrons

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8
Q

what does non-polar covalent bond mean?

A

covalent bonds where the two electrons are shared equally

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9
Q

when do non polar covalent bonds happen?

A

when two atoms in a covalent bond have the same electronegativity

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10
Q

what is polar covalent bonds?

A

covalent bonds where the two electrons are not shared equally

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11
Q

when do polar covalent bonds happen?

A

when 2 atoms in a covalent bond have a different electronegativity

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12
Q

describe linear shape

A

bonding pairs: 2
lone pairs: 0
bond angle: 180

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13
Q

describe trigonal planer

A

bonding pairs: 3
lone pairs: 0
bond angle: 120

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14
Q

describe bent (3)

A

bonding pairs: 2
lone pairs: 1
bond angle: 118

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15
Q

describe tetrahedral

A

bonding pairs: 4
lone pairs: 0
bond angle: 109.5

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16
Q

describe trigonal pyramidal

A

bonding pairs: 3
lone pairs: 1
bond angle: 107

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17
Q

describe bent (4)

A

bonding pairs: 2
lone pairs: 2
bond angle: 104.5

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18
Q

describe trigonal bipyramidal

A

bonding pairs: 5
lone pairs: 0
bond angle: 120 & 90

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19
Q

describe see-saw

A

bonding pairs: 4
lone pairs: 1
bond angle: 119 & 89

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20
Q

describe t shape

A

bonding pairs: 3
lone pairs: 2
bond angle: 89 or 120

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21
Q

describe octahedral

A

bonding pairs: 6
lone pairs: 0
bond angle: 90

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22
Q

describe square pyramid

A

bonding pairs: 5
lone pairs: 1
bond angle: 89

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23
Q

describe square planer

A

bonding pairs: 4
lone pairs: 2
bond angle: 90

24
Q

ionic bonding meaning

A

the electrostatic force of attraction between positively and negatively charged ions in a lattice, metal & non metal

25
Q

formation of ions

A

electrons transferred between atoms. enough electrons lost or gained to empty or fill outer energy level of each atom

26
Q

covalent bond

A

the attraction of two adjacent nuclei for a shared electron pair

27
Q

co-ordinate bond (dative covalent)

A

a covalent bond where both electrons in the shared pair originate from one atom

28
Q

strengths of covalent bonds

A

-the shorter the bond the stronger the bond

  • single bonds < double bonds < triple bonds
29
Q

metallic bonds

A

attraction between postive metal ions and negative delocalised electrons

30
Q

strength of metallic bonding

A

the higher the charge on the positive ion and the smaller the ion the stronger the metallic bonding

31
Q
A
32
Q

what are van der waals’ forces

A
  • present in ALL molecular substances
  • occur because the electrons are constantly moving around
  • the bigger the molecule (more electrons) the greater the Van der Waals forces
33
Q

what is permanent dipole dipole attraction

A

permanent dipole dipole attraction between polar molecules

note: only permanent dipole dipole attractions between polar molecules. Some molecules are non popular but contain polar bonds - these do not have permament dipole dipole attractions

34
Q

what is hydrogen bonding

A

special case of permanent dipole dipole attractions - where an H atom is bonded to a very electronegative atom.

E.g HF, H2O, NH3.

The polar bond between the H and N/O/F leaves the H nucleus exposed as H only has one electron

Therefore strong attraction from lone pair on the N/O/F molecule to the exposed H nucleus of another molecule

This is simply a strong intermolecular forces - not a bond.

35
Q

Strength of intermolecular forces

A

H-bonding > permanent dipole dipole attraction > Van der Waals

36
Q

What is monatomic substances

A

Group 0 elements

37
Q

What is the structure of monatomic

A

Individual atoms with very weak forces between them

38
Q

Melting point and boiling points of monatomic

A

Very weak forces between atoms

39
Q

Does monatomic conduct

A

Do not conduct - no charged particles that can move - atoms are neutral

40
Q

Is monatomic soluble

A

Insoluble

41
Q

Substance of simple molecule

A

Pure Elements and non metal w non metal

42
Q

Structure of similiar molecular

A

Individual molecules with weak forced between them (atoms within molecules are joined by covalent bonds)

43
Q

Melting point and boiling point of simple molecular

A

Low, weak forces between the molecules

note: the atoms within the molecules are held together by strong covalent bonds but there do not break when molecules melt/boil

44
Q

Conductivity it simple molecular

A

Do not conduct
No charged particles that can move - molecules are neutral

45
Q

Giant covalent (macromolecular) structure

A

Lattice structure in which all atoms are joined to others by covalent bonds

46
Q

Melting points and boiling points of giant covalent (macromolecular)

A

very high - need to break many string covalent bonds

47
Q

giant covalent conductivity (macromolecular)

A

do not conduct bc molecular substances do not conduct electricity because molecules are neutral - no mobile charger electrons/ions

Except graphite because it has moving ions between the different layers

48
Q

Ionic structure

A

Lattice structure of positive and negatively charged ions (ions are held together by the attraction between the + and - ions also known as an electrostatic attractive force between ions)

49
Q

Melting & boiling points for ionic

A

Strong electrostatic attraction between positive and negative ions

50
Q

Ionic conductivity

A

Can conduct when dissolved as ions can move

But cannot conduct as solids as ions cant move

51
Q

Ionic solubility

A

Soluble usually

52
Q

Metallic structure

A

Lattice structure of metal ions with outer shell electrons free to move through the structure

53
Q

Metallic melting & boiling points

A

high - strong electron static attraction between positive metal ions and delocalised negative electrons

54
Q

Metallic conductivity

A

Outer shell electrons are free to move through

55
Q

Metallic solubility

A

Insoluble (but some react with water)

56
Q

how do van der waals forces arise between molecules

A

electrons are constantly moving around

induces a dipole in another molecule

induced temporary attraction

physical chem (5 decks)

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