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As Chemistry (Year 1) > 3P-Bonding > Flashcards

3P-Bonding Flashcards

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1
Q

What’s ionic bonding

A

electrostatic attraction between oppositely charged ions in a lattice.

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2
Q

What’s a single covalent bond and multiple bonds eg double bonds

A

Contains one shared pair of electrons
Or multiple pairs of shared electrons eg 2 pairs for double bonds

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3
Q

What are coordinate or dative covalent bonds and how are they represented

A

Contain a shared pair of electrons with both electrons supplied by one atom
Drawn with an arrow

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4
Q

What’s metallic bonding

A

involves attraction between delocalised electrons and positive ions arranged in a lattice

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5
Q

What are the crystal structures and examples of them

A

Ionic eg sodium chloride
Metallic eg magnesium
Macromolecular (giant covalent) eg graphite, diamond
Molecular eg ice, iodine

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6
Q

What’s the melting point, solubility in water and conductivity of ionically bonded substances

A

High mps and bps- giant lattice structure, lots of energy needed to overcome
Solubility in water- good
Conductive- only when aqueous or molten, ions are free to move carrying the charge

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7
Q

What’s the melting point solubility in water and conductivity of covalently bonded structures

A

Low mps and bps- weak intermolecular forces, easy to overcome
Solubility in water- poor/insoluble
Not conductive- molecules aren’t ions

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8
Q

Melting points solubility in water and conductivity of metallically bonded structures

A

High mps and bps- strong attraction between metal ions and delocalised sea of electrons in a giant structure
Solubility in water- insoluble
Conductive- delocalised electrons free to move through structure carrying charge

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9
Q

Other properties of metallically bonded substances

A

Heat conductor- ions packed closely, high thermal conductivity
Malleable and ductile- can be moulded into shape, drawn into wires

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10
Q

Factors effecting strength of ionic covalent or metallic bonds

A

Atomic radius, larger radius less attraction to nucleus
Charge, larger, more electrons shared or transferred so greater attraction

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11
Q

How much energy do different states have

A

Solid- little energy, particles vibrate around a fixed point
Liquid- moderate energy, particles still touching but can flow
Gas- lots of energy, particles bounce off eachother

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12
Q

What’s the name and bonding angle for a molecule with 2 bonding pairs of electrons

A

Linear
180°

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13
Q

What’s the name and bonding angle of a molecule with 3 bonding pairs of electrons

A

Trigonal planar
120°

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14
Q

What’s the name and angle of a molecule with 4 pairs of bonding electrons

A

Tetrahedral
109.5°

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15
Q

What’s the name and angle of a molecule with 5 pairs of bonding electrons

A

Trigonal bipyrimidal
120° (between back and forward atom)
90° (between atoms on same plane)

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16
Q

What’s the name and angle of a molecule with 6 bonding pairs of electrons

A

Octahedral
90°

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17
Q

Why do pairs of electrons organise themselves as far as possible from eachother

A

Due to repulsion

18
Q

In order of most repulsive to least repulsive list whether lone pair or bond pair electrons are most repulsive and why

A

Lone pair-Lone pair (pulled closer to nucleus, more repulsive)
Lone pair-Bond pair
Bond pair-Bond pair

19
Q

How much does a bond angle reduce with one lone pair

A

2.5°

20
Q

What’s the name and bond angle of a molecule with 3 bonding pairs and 1 lone pair of electrons

A

Trigonal pyramidal
107°

21
Q

What’s the name and bonding angle of a molecule with 2 bonding pairs and 2 lone pairs of electrons

A

Bent
104.5°

22
Q

What are the changes of state

A

Solid to liquid, melting
Liquid to solid, freezing
Liquid to gas, boiling
Gas to liquid, condensing
Solid to gas, sublimation
Gas to solid, deposition

23
Q

What’s electronegativity

A

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

24
Q

How to know if a molecule is polar

A

The polar bonds will act unsymetrically and elements will have different electronegativities

25
Q

Even if a molecule has polar bonds the molecule may not be polar why

A

The polar bonds may act symmetrically with equal electronegativity

26
Q

What does a polar molecule possess

A

A permanent dipole

27
Q

What shows a polar bond

A

An arrow with a line through it

28
Q

What’s the trend in electronegativity across a period

A

Increases, increase in number of protons, more attraction, similar shielding

29
Q

What’s the trend of electronegativity down a group

A

Decreases, larger atomic radius, shielding, less attraction for shared pair of electrons to nucleus

30
Q

What are the S+ and S- regions of a polar molecule

A

S+, atom has less attraction, electron deficient
S-, atom has a stronger attraction, electron sufficient

31
Q

What are induced dipole-dipole forces and how are they formed (van der waals, london dispersion)

A

Occur between all molecules
Weakest intermolecular force
Between noble gas atoms

Electrons move randomly, electron density changes at parts of molecule (s+ and s- regions), formation of a temporary dipole, form induced dipoles in neighbouring molecules

32
Q

What are permanent dipole-dipole forces

A

Occur between polar molecules, add to induced dipoles (van der waals) present

33
Q

What are hydrogen bonds

A

Occurs in molecules where a hydrogen atom is attracted to the lone pair of electrons on either nitrogen, oxygen or fluorine (NOF) of another molecule
Strongest intermolecular forces

34
Q

What do you need to include when drawing hydrogen bonds

A

Include the S+ and S- sides
Include dashes to show the bonds
Include the lone pair of electrons

35
Q

What happens to melting and boiling points when intermolecular forces become stronger

A

Increase

36
Q

How do hydrogen bonds cause anomalously high boiling points

A

Hydrogen bonds are in addition to induced dipoles and more forces this need more energy to overcome

37
Q

Why is the density of ice low

A

Hydrogen bonds cause water molecules to be far apart, gaps in lattice

38
Q

How does a higher Mr effect the strength of intermolecular forces

A

Higher Mr, more electrons, stronger van der waals forces between molecules

39
Q

How do isomers effect strength of intermolecular forces

A

Isomers which allow molecules to be packed closely have stronger induced dipoles

40
Q

What’s the name and the bonding angle of a molecule with 4 bonding pairs and 2 lone pairs

A

Square planar
90°

As Chemistry (Year 1) (16 decks)

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