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IB Chemistry HL > Ionic Bonding > Flashcards

Ionic Bonding Flashcards

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1
Q

Ionic bonds

A

bonding due to electrostatic attraction between cations and anions

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2
Q

covalent bonds

A

bonding due to electrostatic attraction between atomic nuclei and a shared pair of electrons

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3
Q

Metallic bonds

A

bonding due to electrostatic attraction between metallic cations and a sea of delocalized electrons

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4
Q

molecular covalent

A

compounds contain atoms held together by covalent bonds.

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5
Q

covalent network

A

formed by networks or chains of atoms or molecules held together by covalent bonds. (ex: diamond)

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6
Q

electrostatic attraction

A

when two particle types have opposite charge and there is mutual attraction.

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7
Q

Melting point

A

temperature at which the solid and liquid forms of a substance can exist in equilibrium. (ionic compounds have ones)

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8
Q

boiling point

A

temperature at which the gas and liquid forms of a substance can exist in equilibrium (ionic compounds have high ones)

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9
Q

volatility

A

a material quality which describes how readily a substance vaporizes. (ionic compounds are not this)

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10
Q

Electrical conductivity

A

ability to carry and electrical charge. Ionic compounds can do this when they are molten or dissolved in solution.

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11
Q

Thermal conductivity

A

ability to transfer heat. Ionic compounds do not do this.

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12
Q

Brittle

A

hard but liable to break or shatter easily. Ionic compounds are this.

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13
Q

corrosion

A

a process by which metals deteriorate through oxidation. Some ionic compounds can do this.

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14
Q

Electronegativity

A

a chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself

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15
Q

Cation

A

positively charged species due to a loss of electrons.

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16
Q

oxidation

A

the loss of electrons

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17
Q

reduction

A

the gain of electrons

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18
Q

anion

A

negatively charged species due to a gain of electrons.

19
Q

redox reaction

A

the coupling of a loss of electrons from one chemical to the gain of electrons by another.

20
Q

OIL RIG

A

oxidation is loss and reduction is gain (of electrons)

21
Q

hydride

A

H3O+, the ion formed when hydrogen ions are in aqueous solution

22
Q

octet rule

A

the tendency of atoms to prefer to have eight electrons in the valence shell.

23
Q

transition elements

A

elements with an incomplete d orbitals

24
Q

Exothermic

A

a process that releases energy

25
Q

Endothermic

A

a process that absorbs energy

26
Q

Polyatomic ions

A

an ion composed of more than one atom.

27
Q

Nitrate

A

NO3 -1

28
Q

ammonium

A

NH4 +

29
Q

hydroxide

A

OH -

30
Q

hydrogencarbonate

A

HCO3 -

31
Q

carbonate

A

CO3 2-

32
Q

Sulfate

A

SO4 2-

33
Q

Phosphate

A

PO4 3-

34
Q

Pauling scale

A

the most commonly used scale to measure relative electronegativity

35
Q

Ionic crystals

A

solids consisting of ions bound together by their electrostatic attraction into a regular lattice.

36
Q

lattice structure

A

the symmetrical three-dimensional structural arrangements of atoms, ions or molecules

37
Q

non-directional bonding

A

due to ionic charges being uniform in all directions, An ion is surrounded by other ion from all the directions.

38
Q

lattice enthalpy

A

a measure of the strength of the forces between the ions in an ionic solid.

39
Q

solubility

A

a measure of the strength of the forces between the ions in an ionic solid. If the attraction between the solvent and the solute is higher than the lattice enthalpy of the compound then it will dissolve.

40
Q

Polar solvent

A

can dissolve polar and ionic compounds

41
Q

Non polar solvent

A

can dissolve non-polar compounds

42
Q

How ionic radius affects lattice enthalpy

A

the higher the ionic radius the lower the lattice enthalpy

43
Q

how ionic charge affects lattice enthalpy

A

the higher the ionic charge the higher the lattice enthalpy

IB Chemistry HL (12 decks)

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