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Chemistry IB > Chemical Bonding and Structure > Flashcards

Chemical Bonding and Structure Flashcards

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1
Q

Hydroxide?

A

OH-

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2
Q

Hydrogen carbonate?

A

HCO3-

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3
Q

Nitrate?

A

NO3-

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4
Q

Carbonate?

A

CO3 2-

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5
Q

Sulfate?

A

SO4 2-

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6
Q

Nitride?

A

n3-

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7
Q

Phosphate?

A

PO4 3-

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8
Q

What is an ionic bond?

A

An ionic bond is an electrostatic attraction between oppositely charged ions.

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9
Q

What is a covalent bond?

A

Covalent bonding occurs when atoms share electrons and a covalent bond is the electrostatic attraction between a shared pair of electrons and the nuclei of the atoms that are bonded.

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10
Q

What is electronegativity?

A

Electronegativity is a measure of the attraction of an atom in a molecule for the electron pair in the covalent bond of which it is a part.

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11
Q

What is a dative bond?

A

Or a coordinate covalent bond?

A coordinate covalent bond is a type of covalent bond in which both electrons come from the same atom

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12
Q

What is the VSEPR theory?

A

Pairs of electrons (electron domains) in the valence (outer) shell of an atom repel each other and will therefore take up positions in space to minimise these repulsions - to be as far apart in space as possible.

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13
Q

What shape would Y-X-Y be?

A

Linear 180 degrees

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14
Q

What shape would XY3 be?

A

Trigonal planer 120 degrees

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15
Q

What shape would XY4 be?

A

Tetrahedral 109.5 degrees

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16
Q

What is the order of strength of repulsion for pairs of electrons?

A

lone pair - lone pair > lone pair - bonding pair > bonding pair - bonding pair
This is because lone pairs are held closer to the central nucleus than are bonding pairs. Lone pairs are on the outer shell of the atom whereas bonded ones are half way between the two atoms. The lone pairs are therefore closer to each other and the bonding pairs than the bonding pairs are to each other. This causes them to repel more.

17
Q

How much do lone pairs decrease the bond angle by?

A

Lone pairs decrease the other bonded angles by 2 or 3 degrees.

18
Q

What is a dipole moment?

A

This is overall polarity of a molecule. So if it has a negative and a negative side, they will cancel out a bit, it is the overall that is the dipole moment, so it will be polar if one is more negative than the other.
Although individual bonds may be polar, a molecule may be non-polar overall, if, because of the symmetry of the molecule, the dipole moments of the individual bonds cancel out.

19
Q

What are allotropes?

A

Allotropes are different forms of the same element. For instance diamond, graphene and fullerenes are all allotropes of carbon.

20
Q

What is the structure of diamond?

A

Diamond has a giant covalent structure. There are no individual molecules - the whole structure, continuing in three dimensions, represents one giant molecule. Each carbon atom is joined to four others in a tetrahedral array, by covalent bonds.
It has a very high melting and boiling point. It does not conduct electricity because all the electrons are held strongly in covalent bonds and are therefore not free to move around in the structure.
It does not dissolve in water because the forces between the atoms are too strong. The energy to break these covalent bonds would not be paid back when the C atoms were solvated.

21
Q

What is the structure of Graphite?

A

Graphite has a giant covalent structure. It has layers and each C is covalently bonded to three others in a trigonal planar array. There are covalent bonds in the layers but only London forces between the layers.
It can conduct electricity but its melting and boiling point are still very high because you have to break 3 covalent bonds.
Each C in graphite contains one ‘p’ orbital, these overlap side on to form a pi delocalised system, extending over the whole layer.

22
Q

What is graphene?

A

One thin layer of graphite.

23
Q

What is C60?

A

This is considered as a molecule rather than as a giant structure. It consists of individual C60 molecules with covalent bonds within the molecule and London Forces between the molecules.
It is insoluble in water but soluble in some organic compounds.
It does no conduct electricity although each Carbon is only bonded to 3 other because of the molecular structure these electrons are not able to move from one molecule to the next.

24
Q

What is silicon dioxide?

A

SiO2, it is a giant covalent structure. It has high melting and boiling points.

25
Q

What is the difference between intermolecular forces and intramolecular forces?

A

Inter is between molecules, intra is in the molecules.

26
Q

What are London forces?

A

London forces are temporary (instantaneous) dipole induced dipole interactions. Electrons in an atom are in constant motion, and at any one time they will not be symmetrically distributed about the nucleus. This results in a temporary (instantaneous) dipole in the atom, which will then induce one in the next atom and they will be attracted to one another.

27
Q

What is the rising scale in strength of intermolecular forces?

A

London dispersion forces > dipole-dipole > hydrogen bonding

28
Q

What is a hydrogen bond?

A

A ONF attached to a hydrogen makes one.

29
Q

What effects the strength of metallic bonds?

A

The higher charge e.g. 2+ will be greater than 1+, and the size of the atom, so the smaller atom will form a stronger bond.

Chemistry IB (9 decks)

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