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physical chem > bonding (3) > Flashcards

bonding (3) Flashcards

(57 cards)

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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

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A

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

24
Q

ionic bonding meaning

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A

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

25
formation of ions
electrons transferred between atoms. enough electrons lost or gained to empty or fill outer energy level of each atom
26
covalent bond
the attraction of two adjacent nuclei for a shared electron pair
27
co-ordinate bond (dative covalent)
a covalent bond where both electrons in the shared pair originate from one atom
28
strengths of covalent bonds
-the shorter the bond the stronger the bond - single bonds < double bonds < triple bonds
29
metallic bonds
strong attraction between postive metal ions and negative delocalised electrons
30
strength of metallic bonding
the higher the charge on the positive ion and the smaller the ion the stronger the metallic bonding
31
what are van der waals’ forces
- 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
32
what is permanent dipole dipole attraction
permanent dipole dipole attraction between polar molecules when they have a large electronegativity difference 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
33
what is hydrogen bonding
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.
34
Strength of intermolecular forces
H-bonding > permanent dipole dipole attraction > Van der Waals
35
What is monatomic substances
Group 0 elements
36
What is the structure of monatomic
Individual atoms with very weak forces between them
37
Melting point and boiling points of monatomic
Very weak forces between atoms
38
Does monatomic conduct
Do not conduct - no charged particles that can move - atoms are neutral
39
Is monatomic soluble
Insoluble
40
Substance of simple molecule
Pure Elements and non metal w non metal
41
Structure of similiar molecular
Individual molecules with weak forced between them (atoms within molecules are joined by covalent bonds)
42
Melting point and boiling point of simple molecular
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
43
Conductivity it simple molecular
Do not conduct No charged particles that can move - molecules are neutral
44
Giant covalent (macromolecular) structure
Lattice structure in which all atoms are joined to others by covalent bonds
45
Melting points and boiling points of giant covalent (macromolecular)
very high - need to break many string covalent bonds
46
giant covalent conductivity (macromolecular)
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
47
Ionic structure
*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)
48
Melting & boiling points for ionic
Strong electrostatic attraction between positive and negative ions
49
Ionic conductivity
Can conduct when dissolved as ions can move But cannot conduct as solids as ions cant move
50
Ionic solubility
Soluble usually
51
Metallic structure
*Lattice structure* of metal ions with outer shell electrons free to move through the structure
52
Metallic melting & boiling points
high - strong electron static attraction between positive metal ions and delocalised negative electrons
53
Metallic conductivity
Outer shell electrons are free to move through
54
Metallic solubility
Insoluble (but some react with water)
55
how do permanent dipole dipole forces arise between molecules
Difference in electronegativity leads to bond polarity and there is an attraction between ∂+ on one molecule and ∂- on another
56
Van der Waals’ forces exist between all molecules. Explain how these forces *arise*
Electron movement in first molecule / temporary dipole Induces a dipole in another molecule (Induced-temporary) attraction or δ+ attracts δ- in different/adjacent molecules
57
Suggest a value for the H−O−O bond angle.
94−105.5°

physical chem (12 decks)

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