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zAS Chemistry > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

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1
Q

What is this bond shape and angle?

A

Linear shape with 180° bond angles

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2
Q

What is this bond shape and angle?

A

Triagonal planar shape and 120° angles.

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3
Q

What is this bond shape and angle?

A

Tetrahedral shape and 109.5° angles,

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4
Q

What is this bond shape and angle?

A

Triagonal bipyramidal shape and 90° or 120° angles.

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5
Q

What is this bond shape and angle?

A

Octahedral shape and 90° angles.

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6
Q

What is this bond shape and angle?

A

Bent shape and 104.5° angles.

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7
Q

What is this bond shape and angle?

A

Triagonal pyramindal shape and 107° angles.

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8
Q

What is this bond shape and angle?

A

Square planar shape and 90° angles.

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9
Q

What holds ionic lattices together?

A

Electrostatic forces between positive and negative ions

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10
Q

What kind of crystal is formed by Oxygen and Fluorine?

A

Molecular

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11
Q

What is bond formed between a lone pair and an ion (normally) called?

A

A dative bond

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12
Q

What are diamond, sand and graphite all examples of?

A

Macromolecular bonding

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13
Q

Why are graphite and graphene great conductors of electricity?

A

Because they have a delocalised electrons which are free to move and carry a current

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14
Q

Why can pure metals easily be bend and hammered into different shapes?

A

Because they have layers of the same size ions which can slide across one another

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15
Q

What is the definition of electronegativity?

A

The power of an atom to withdraw electrons in a covalent bonds

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16
Q

What is the pattern for increasing Van der Waals forces?

A

The further across the period you go and the further down the group you go as the number of electrons increases

17
Q

What are the conditions for increasing diople forces?

A

The greater the electronegativity difference between atoms, the greater the partial charges and strength of the diople forces between molecules

18
Q

What are the conditions for hydrogen bonding?

A

Where hydrogen is bonded with either Oxygen, Nitrogen or Fluorine

19
Q

Why is ice less dense than water?

A

Because the hydrogen bonding between the water molecules form a regular lattice structure which spaces the molecules apart.

20
Q

Which metals will have higher melting points?

A

Metals with higher numbers of outer shell electrons as they have stronger electrostatic forces between the ions and electrons

zAS Chemistry (16 decks)

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