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CHEM > 1.3 Covalent Bonding > Flashcards

1.3 Covalent Bonding Flashcards

1
Q

shape of beryllium chloride

A

linear

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2
Q

shape of H2O

A

bent

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3
Q

shape of boron trifluoride

A

triognal planar

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4
Q

electron pair repulsion theory

A

electron pairs are negatively charged and repel each other so are arranged to minimise repulsion and maximise separation

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5
Q

dative covalent bond

A

when an atom supplies both electrons in the formation of a covalent bond

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6
Q

when an atom supplies both electrons in the formation of a covalent bond

A

dative covalent bond

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7
Q

bonding pair of electrons

A

two electrons shared in a covalent bond

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8
Q

lone pair

A

held closer to the central atom, so they have a greater repulsion than bonding pairs

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9
Q

held closer to the central atom, so they have a greater repulsion than bonding pairs

A

lone pair

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10
Q

repulsion continuum

A

LP-LP greatest repulsion → LP-BP → BP-BP weakest repulsion

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11
Q

bonding/lone pair equation

A

electron pairs = (Number of electrons of the central atom + number of atoms attached) /2

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12
Q

2 BPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: linear
  • molecule shape: linear
  • angle: 180
  • shape: Be-Cl-Be
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13
Q

3 BPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: trigonal planar
  • molecule shape: trigonal planar
  • angle: 120
  • shape: pictured
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14
Q

4 BPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: tetrahedral
  • molecule shape: tetrahedral
  • angle: 109.5
  • shape: pictured
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15
Q

5 BPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: trigonal bipyramidal
  • molecule shape: trigonal bipyramidal
  • angle: 90, 120, 180
  • shape: pictured
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16
Q

6 BPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: octahedral
  • molecule shape: octahedral
  • angle: 90
  • shape: pictured
17
Q

2 BPs 2 LPs:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: tetrahedral
  • molecule shape: bent angular
  • angle: 104.5
  • shape: pictured
18
Q

3 BPs 1 LP:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: tetrahedral
  • molecule shape: trigonal pyramidal
  • angle: 107
  • shape: pictured
19
Q

4 BPs 2 LP:

  • electron pair arrangement
  • molecule shape
  • angle in degrees
  • shape
A
  • electron pairs: octahedral
  • molecule shape: square planar
  • angle: 90
  • shape: pictured
20
Q

bond angle for lone paired atoms equation

A

109 - (2.5 x number of lone pairs)

21
Q

what do to do electron number when there is a negative ion

A

add an electron

22
Q

what do to do electron number when there is a positive ion

A

remove an electron

23
Q

bond angle of BF3

24
Q

shape of NH4^+

A

molecule is tetrahedral, electron pairs are tetrahedral

25
Q

shape of NH3

A

molecule is pyramidal, electron pairs are tetrahedral

26
Q

shape of AlH4^-

A

molecule is tetrahedral, electron pairs are tetrahedral

27
Q

shape of SF6

A

molecule is octahedral, electron pairs are octahedral

28
Q

shape of BF3

A

molecule is trigonal planar, electron pairs are trigonal planar

29
Q

shape of BeCl2

A

molecule is linear, electron pairs are linear

30
Q

shape of IF4^-

A

molecule is square planar, electron pairs are octahedral

CHEM (10 decks)

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