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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Ionic bonding definition

A

Electrostatic attraction between oppositely charged ions formed by electron transfer

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2
Q

Ionic bonding structure

A

Giant ionic lattice

Crystalline solid

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3
Q

Ionic bonding examples

A 
Sodium Chloride (NaCl)
Magnesium Oxide (MgO)
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4
Q

Ionic bonding melting and boiling points

A

High MP and BP
Giant lattice of ions with many strong electrostatic forces between oppositely charged ions
The smaller the ion and the higher the charge, the stronger the bond

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5
Q

Ionic binding solubility

A

Generally good
Water molecules surround ions that have broken out of lattice
When water molecule hits ionic lattice, can knock ions off to surround
Aluminium oxide (Al2O3) not soluble in water as electrostatic attraction too strong

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6
Q

ionic bonding conductivity

A

Do not conduct electricity when solid as ions cannot move and are fixed in a lattice
Conduct electricity when molten or in aqueous solution as ions are free to move and carry charge

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7
Q

covalent bonding definition

A

Shared pair of electrons

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8
Q

covalent bonding structure

A 
Simple molecular
With intermolecular forces between molecules
Mostly gases and liquids
Macromolecular
Giant molecular structures
solids
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9
Q

covalent bonding examples

A 
Simple molecular
Iodine (I2)
ice/water (H2O)
Carbon dioxide (CO2)
Methane (CH4)
Macromolecular
Diamond (carbon bonds)
Graphite (carbon bonds)
Silicon dioxide (SiO2)
Silicon (silicon bonds)
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10
Q

covalent bonding melting and boiling points

A

Simple molecular
Low due to weak intermolecular forces between molecules
Macromolecular
High due to many strong covalent bonds in structure

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11
Q

covalent bonding solubility

A

Simple molecular
Generally poor
Macromolecular
insoluble

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12
Q

covalent bonding conductivity

A

Simple molecular
Poor as no ions free to conduct and electrons are fixed in place (localised)
Macromolecular
Most compounds poor as no ions and only localised electrons
Graphite good as free electrons between layers

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13
Q

Dative covalent bonding

A

Forms when shared pair of electrons in covalent bond comes from only one of the bonding atoms
Also called co-ordinate bond
Direction of arrow goes from atom providing lone pair to atom that is deficient

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14
Q

common examples of dative covalent bonding

A

NH4 +
H3O +
NH3BCl3

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15
Q

Diamond

A

Each carbon atom is bonded to four other carbon atoms by strong covalent bonds creating a giant covalent structure.
Very hard due to the many strong covalent bonds.
Does not conduct electricity as no delocalised electrons.
High melting point
Very rigid structure so vibrations can easily carry vibrations through the structure so diamond is a good thermal conductor.

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16
Q

Graphite

A

Each carbon atom is bonded to 3 other carbon atoms creating giant covalent structure.
High melting point.
Insoluble in solvents
Soft as carbon atoms form hexagonal rings with each layer held together by weak intermolecular forces. Layers can slide over each other, making it a good lubricant.
Conducts electricity due to delocalised electrons that can move freely.

17
Q

metallic bonding definition

A

Electrostatic force of attraction between positive metal ions and delocalised electrons

18
Q

metallic bonding structure

A

Giant metallic lattice

19
Q

metallic bonding examples

A

All metals

20
Q

Properties of metallic bonding

A

Shiny metal
Malleable as positive ions are all identical so planes of ions can slide over one another
Attractive forces are the same whichever ions are adjacent

21
Q

metallic bonding melting and boiling points

A

High due to strong electrostatic forces of attraction

Large rectangular structure

22
Q

metallic bonding solubility

A

Insoluble in water

React with water to form metal oxides

23
Q

metallic bonding electrical conductivity

A

Good as delocalised electrons can move throughout structure

24
Q

metallic bonding heat conductivity

A

High as particles can move and are close enough together to transfer thermal energy
Silver excellent conductor used in rear window defrosters in cars

25
Q

Factors affecting strength of bonding

A 
Number of protons:
More protons
Stronger bond
Number of delocalised electrons per atom:
More electrons
Stronger bond
Size of ion:
Smaller ion
Stronger bond
26
Q

Electronegativity definition

A

Ability of an atom to attract a bonding pair of electrons in a covalent bond
Measured on Pauling Scale (0-4)
F, O, N and Cl are the most electronegative atoms

27
Q

Factors affecting electronegativity

A

Distance of bonding electrons from nucleus
Can be taken to be the same as atomic radius
Nuclear charge
Greater nuclear charge
Decreases atomic radius
Increases electronegativity
Shielding
Inner electrons shield attractive power of nucleus

28
Q

Trend across a period

electronegativity

A

Atomic radius decreases
Stronger attraction
Nuclear charge increases
Electronegativity increases

29
Q

Trend down a group

electronegativity

A

Atomic radius increases
Shielding increases
Electronegativity decreases

30
Q

Intermediate bonding

A

Compounds containing elements with a small electronegativity difference will be purely covalent
Compounds containing elements with large electronegativity difference (>1.7) will be ionic
Polar covalent bond forms when elements have electronegativity difference of 0.3-1.7

31
Q

Polar and non polar molecules

A 
Symmetrical molecules (all bonds identical and no lone pairs) will never be polar
Individual dipoles cancel out so no net dipole, non polar
32
Q

Intermolecular forces

A

Induced dipole-dipole forces
Permanent dipole-dipole forces
Hydrogen bonding

33
Q

Van der waals forces

A

Also called transient forces and induced dipole-dipole interactions
Occur between all molecular substances and noble gases
Do not occur in ionic substances
Movement of electron clouds cause partial charges to change rapidly creating temporary dipoles. These partial charges exert force on nearby molecules resulting in induced dipole interaction

34
Q

Factors affecting van der waals

A

More electrons increases chance that temporary dipole will form
Increases strength of van der waals forces between molecules

35
Q

Permanent dipole-dipole forces

A

Occur only between polar molecules
Stronger than van der waals forces
Have permanent dipole within molecule
The delta+ end of one dipole is attracted to delta- end of dipole on another molecule

36
Q

Hydrogen bonding

A

Occurs in compounds that have a hydrogen atom attached to N, O or F
Large electronegativity difference
Stronger than van der waals and permanent dipole-dipole
Weaker than any intramolecular interactions

Chemistry (7 decks)

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