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IB chemistry > Topic 4: Chemical bonding and structure > Flashcards

Topic 4: Chemical bonding and structure Flashcards

1
Q

What is an ionic compound?

A

The electrostatic attraction between oppositely charged ions

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2
Q

What is an ion?

A

A charged species that is formed when electrons are transferred from one atom to another

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3
Q

What is the structure of ionic compounds?

A

Lattice

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4
Q

The octet rule

A

Elements tend to lose or gain electrons or share electrons in order to acquire a noble gas configuration

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5
Q

Electrical conductivity of ionic impounds

A

It cannot conduct electricity in the solid state, but it can conduct electricity when molten or in an aqueous solution

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6
Q

Solubility of ionic compounds

A

Soluble in polar solvents (eg: water) but not non polar solvents. Ions are attracted to ester molecules and are pulled away from the lattice and the separate ions are hydrated by water molecules

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7
Q

Volatility meaning

A

The tendency of a substance to vaporise

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8
Q

Volatility of ionic compounds

A

Ionic compounds have a strong electrostatic force of attraction between oppositely charged ions, making the volatility low

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9
Q

Why are ionic compounds not soluble in non-polar solvents?

A

There is no attraction between the non-polar solvent and the ions of the lattice

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10
Q

Brittleness of ionic compounds, why?

A

Ionic compounds shatter when they are hit, because when they are suddenly hit with a force, the ions shift, so that like charges become situated next to each other, and they repel each other so the lattice structure breaks apart

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11
Q

Electronegativity definition

A

The power of an atom in a molecule to attract electrons to itself

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12
Q

Electronegativity trend

A

Lowest in in lower left and highest in upper right

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13
Q

Ionic compounds is usually between a

A

A metal + a non-metal

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14
Q

Covalent compounds is usually between two

A

Non-metals

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15
Q

Ionic compounds Electronegativity difference

A

More than 1.8

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16
Q

Covalent compounds Electronegativity difference

A

Equal to or less than 1.8

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17
Q

Polar covalent compounds Electronegativity difference

A

Between 0 and 1.8 (non inclusive)

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18
Q

Metals ions charge

A

Usually Positive

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19
Q

Non-metals charge

A

Usually negative

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20
Q

Atoms that are stable with less than 8 electrons in the valence shell

A

Hydrogen, boron, beryllium

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21
Q

Suffix for anions in an ionic compound, give an example

A

-ide (eg:chloride)

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22
Q

Oxoanions meaning

A

Polyatomic ions containing oxygen (eg: NO3 -)

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23
Q

Why is NaCl described as having a local octahedral geometry?

A

Each sodium ion is surrounded by six chloride ions and each chloride ion is surrounded by six sodium ions

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24
Q

Formula for lithium

A

Li +

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25
Q

Formula for sodium

A

Na +

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26
Q

Formula for potassium

A

K +

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27
Q

Formula for caesium

A

Cs +

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28
Q

Formula for Calcium

A

Ca 2+

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29
Q

Formula for Magnesium

A

Mg 2+

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30
Q

Formula for aluminium

A

Al 3+

31
Q

Formula for zinc ion

A

Zn 2+

32
Q

Formula for copper (II)

A

Cu 2+

33
Q

Formula for lead

A

Pb 2+

34
Q

Formula for iron (II)

A

Fe 2+

35
Q

Formula for iron (III)

A

Fe 3+

36
Q

Formula for fluoride

A

F -

37
Q

Formula for chloride

A

Cl -

38
Q

Sulfide

A

S 2-

39
Q

Formula for bromide

A

Br -

40
Q

Formula for iodide

A

I -

41
Q

Formula for oxide

A

O 2-

42
Q

Nitride

A

N 3-

43
Q

What has both covalent bonding and ionic bonding?

A

An ionic compound containing polyatomic ions

44
Q

Phosphide

A

P 3-

45
Q

What are polyatomic ions?

A

Ions that consist of more than one atom

46
Q

Formula of ammonia

A

NH3

47
Q

Formula of hydroxide

A

OH -

48
Q

Formula of amonium

A

NH4 +

49
Q

Formula of nitrite

A

NO2 -

50
Q

Formula of nitrate

A

NO3 -

51
Q

Formula of hydrogen carbonate

A

HCO3 -

52
Q

Formula of sulphate

A

SO4 2-

53
Q

Formula of carbonate

A

CO3 2-

54
Q

Sulfite

A

SO3 2-

55
Q

Formula for phosphate

A

PO4 3-

56
Q

Formula for chlorite

A

ClO2 -

57
Q

Formula for perchlorate

A

ClO4 -

58
Q

Formula for chlorate

A

ClO3 -

59
Q

Formula for hypochlorite

A

ClO -

60
Q

The melting and boiling points of ionic compounds–why?

A

Relatively high, because of the strong forces of attraction between ions in a lattice structure

61
Q

Volatility

A

How easy a substance vaporizes (boiling point)

62
Q

What is hydration?

A

When seperated ions are surrounded by water molecules

63
Q

Examples of non-polar solvents

A

Hexane, propane

64
Q

Do ionic compounds conduct electricity? Why/why not?

A

They do not in solid form because ions are held in fixed positions in the lattice structure. When an ionic compound is dissolved/molten, ions are free to move and carry an electric current

65
Q

Why do ionic compounds shatter when force is applied?

A

When a force is applied, the ions move and the force of repulsion between of the same charge causes the lattice structure to split and fracture.

66
Q

Why can some ionic compounds dissolve in water?

A

The partial charges of water molecules are attracted to the oppositely charged ions in the lattice structure. The ions break off and are surrounded by water molecules. If the forces between the ions and water molecules are stronger than the attraction between the ions themselves, then the ionic compound is soluble.

67
Q

Define covalent bonding

A

The electrostatic attraction between positively charged nuclei and shared pairs of bonding electrons

68
Q

Why are longer bonds weaker than shorter bonds?

A

Because of the increased distance between the nuclei and the shared pairs of electrons, which results in a weaker electrostatic attraction between the atoms

69
Q

Why are multiple bonds stronger than a single bond?

A

Multiple bonds involve more shared electrons between the atoms, so the electrostatic attraction is greater

70
Q

How do you know if a covalent bond is a coordinate covalent bond?

A

If the bonding electrons come from one atom (in a regular covalent bond, electrons come from both atoms)

71
Q

Example of a coordinate covalent bond?

A

CO (carbon monoxide)
NH4 + (Ammonium ion)
H3O + (Hydronium ion)

72
Q

Aluminium chloride is a bond between a metal and non-metal–why is it not an ionic bond?

A

Aluminium chloride is electron deficient, it still needs two electrons to complete the octet in the outer shell of the aluminium atom, which creates a polar covalent bond

73
Q

What is a dimer?

A

A larger molecule formed composed of two smaller, identical molecules and can be linked by coordinate covalent bonds or hydrogen bonds

IB chemistry (11 decks)

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