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Chemistry (AS) > Bonding > Flashcards

Bonding Flashcards

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1
Q

Structure, Angle & example of a molecule:
2 Bonding pairs with 0 lone pairs

A

Linear, 180, CO2

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2
Q

Structure, Angle & example of a molecule:
3 Bonding pairs with 0 lone pairs

A

Trigonal Planar, 120, BF3

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3
Q

Structure, Angle & example of a molecule:
2 Bonding pairs with 1 lone pairs

A

Bent, 118 (between bonding pairs) , NO2

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4
Q

Structure, Angle & example of a molecule:
4 Bonding pairs with 0 lone pairs

A

Tetrahedral, 109.5, CH4

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5
Q

Structure, Angle & example of a molecule:
3 Bonding pairs with 1 lone pairs

A

Trigonal Pyramid, 107, NH3

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6
Q

Structure, Angle & example of a molecule:
2 Bonding pairs with 2 lone pairs

A

Bent, 104.5 (between bonding pairs) , H2O

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7
Q

Structure, Angle & example of a molecule:
5 Bonding pairs with 0 lone pairs

A

Trigonal Bipyramid, 120 (Between bonding pairs on XY plane) 90 (between bonding pairs on ZY plane) PF5

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8
Q

Structure, Angle & example of a molecule:
4 Bonding pairs with 1 lone pairs

A

Seesaw, 118 (between bonding pairs on ZY plane) 89 (between bonding pairs ZX plane) SF4

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9
Q

Structure, Angle & example of a molecule:
3 Bonding pairs with 2 lone pairs (2 formats)

A

1) Trigonal Planar, 120 (with 2 lone pairs on the ZY plane) ICl3
2)T-Shaped 89 (between bonding pairs ZX plane) with 2 lone pairs on the top in the ZX plane ICl3

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10
Q

Structure, Angle & example of a molecule:
6 Bonding pairs with 0 lone pairs

A

Octahedral, 90 between every molecule , SF6

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11
Q

Structure, Angle & example of a molecule:
5 Bonding pairs with 1 lone pairs

A

Distorted square Pyramid, (89 between XY plane to the point in the positive Z axis ) with lone pair on the negative z axis, XeF5

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12
Q

Structure, Angle & example of a molecule:
4 Bonding pairs with 2 lone pairs

A

Square Planar, 90 between 4 bonding pairs in xy plane with a lone pair stationed both he positive and negative z axis, XeF4

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13
Q

What is a Coordinate Bond

A

Where 1 atom donates 2 electrons to form a covalent bond

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14
Q

Hydrogen bonding occurs between

A

H-F
H-N
H-O
Bonds

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15
Q

What is an instantaneous Diople?

A

When the electron density is fluctuating in a molecule that is unpolarised
that oppositely charged dipoles are formed either side of the molecule
Occurs between similar electronegative bonds

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16
Q

Draw the shape of the molecule NCl4+ , name the shape and corresponding bond angles

Explain why it is that bond angle

A

tetrahedral — 109.5

4Bp and 0Lp , electron pairs repel equally & chlorines are stationed as far as part as possible from one another

17
Q
A

D

F2 has no polar bonds
CBr4 CO2 and PF3 do
CBr4 and CO2 have symmetrical arrangement while PF3 doesn’t

18
Q

Explain why MgCl2 has a high melting point

A

Large intermolecular forces of electrostatic attraction between oppositely charged ions in a regular arrangement

That require a lot of energy to overcome

19
Q

Explain how melting or dissolving MgCl2 can conduct electricity

A

Melting or dislodging releases Mg2+ and Cl- ions

These charged ions can move and carry a charge.

Conducting electricity

20
Q
A

Carbon Atoms arranged in hexagonal sheets of hexagons

Each carbon atom is covalently bonded to 3 other carbon atoms

The 4th outer electron is delocalised

Sheets of carbon held together by Van Dee Waal forces

21
Q

Why does graphite have a high melting point

A

To melt graphite you have to break strong covalent bonds, which take along of energy

22
Q

Explain why CHCl3 is polar while CCl4 is not polar

A
23
Q

Explain the Structure of Ice

A

Molecular Crystalline structure

Each water molecule is surrounded by four neighbouring water molecules, forming a lattice, each of them are hydrogen bonded to one another

24
Q

Explain why ice has a lower density then water

A

Regular lattice arrangement contains more hydrogen bonds then liquid water

Crystalline structure holds molecules further apart from each other on average then in liquid water

Meaning a decrease in mass per unit volume

25
Q

Draw a Water molecule

A
26
Q

Justify why H2O has a bond angle of 104.5 degrees

A

Bonding pair - lone pair replulsion is greater then bonding pair - bonding pair repulsion.

As electrons pairs repel to be as far away from each other as possible this causes the bond angle to reduce from 180 to 118 with 1 lone pair of electrons

2 lone pair of electrons reduce the angle between the bonding pairs even more as lone pair lone pair repulsion is stronger then bonding pair lone pair from 118 to 104.5.

27
Q

Draw the Hydrogen Bonding between two molecules of Ethanol

A

Chemistry (AS) (16 decks)

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