bonding and structure Flashcards

1
Q

what is the definition of a covalent bond?

A

the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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2
Q

what is a valence electron?

A

an electron on the outer shell

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3
Q

what is a dative covalent bond?

A

a dative bond is a covalent bond where only one of the bonded atoms donates both electrons being shared

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4
Q

what does a stick in a displayed formula represent?

A

a covalent bond

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5
Q

how many degreees does a lone pair change the bond angle by?

A

2.5°

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6
Q

4 bonding pairs and no lone pairs?

A

tetrahedral
bond angles of 109.5°

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7
Q

3 bonding pairs and 1 lone pair?

A

pyramidal
bond angles of 107°

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8
Q

2 bonding pairs and 2 lone pairs?

A

v-shaped
104.5°

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9
Q

3 bonding pairs?

A

trigonal planar
120°

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10
Q

2 bonding pairs?

A

linear
180°

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11
Q

6 bonding pairs?

A

octahedral
90°

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12
Q

what are the election repulsion rules?

A

lone pairs repel more than bonded pairs

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13
Q

what are the election repulsion rules?

A

lone pairs repel more than bonded pairs

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14
Q

give the order of strength of intermolecular forces

A

hydrogen bonding > permanent dipole - dipole > induced dipole-dipole

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15
Q

why does an induced dipole-dipole interaction increase in strength?

A

more electrons/larger molecule size or less branched carbon chains

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16
Q

what is electronegativity?

A

the ability of an atom to attract the bonding elections in a covalent bond

17
Q

define a polarbond

A

the convent bond between atoms with different electronegativity

18
Q

define a hydrogen bond

A

the intermolecular force between the lone pair of a N, O or F of an NH, OH or FH with the H atom of NH, OH or FH in a neighbouring molecule

19
Q

2 bonding pairs and 1 lone pair?

A

v-shaped
117.5

20
Q

define a polar molecule

A

an unsymmetrical molecule whose dipoles don’t cancel out

21
Q

what are 2 anomalous properties of water?

A
  1. a higher than expected melting and boiling point
  2. solid water is less dense than liquid water
22
Q

why is solid water less dense than liquid water?

A

hydrogen bonding holds water molecules in an open lattice

23
Q

why does water have a higher than expected boiling point?

A

strong hydrogen bonding requires a lot of energy to break the intermolecular forves

24
Q

what is ionic bonding?

A

the strong electrostatic attraction between oppositely charged ions

25
Q

why do solid ionic substances not conduct?

A

the ions are fixed in a lattice and cannot move

26
Q

how do aqueous and molten ionic substances conduct electricity?

A

the ions are free to move

27
Q

what is metallic bonding?

A

the strong electrostatic attraction between positive ions and delocalised electrons

28
Q

how do metals conduct electricity?

A

delocalised electrons can move and conduct electricity