Chapter 6 Flashcards

1
Q

What is the shape and properties of group two?

A

linear, 180°, 2 bond pair and no lone pairs

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2
Q

What is the shape and properties of group 3?

A

Trigonal planar, 120°, 3 bond pairs and no lone pairs

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3
Q

What is the properties and shape of group 4?

A

Tetrahedral, 109.5°, 4 bond pairs and no lone pairs

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4
Q

What is the shape and properties of group 5?

A

Pyramidal, 107º, 3 bond pairs and one one pair

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5
Q

What is the shape and properties of group 6?

A

Non-linear, 104.5°, 2 bond pair 2 lone pair

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6
Q

Why are electrons equally spaced out?

A

Repulsion’s are equal

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7
Q

What happens to the shape it lone pairs are present?

A

Shape is distorted

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8
Q

Why is the shape distorted with the addition of lone pairs?

A

Extra repulsion is caused by lone pairs

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9
Q

How much do lone pairs push bond angle down by?

A

2.5°

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10
Q

How many bonding pairs does an octahedral have? What is the bond angle

A

6 pairs, 90°

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11
Q

What is electronegativity?

A

A measure of the tendency of an atom to attract a bonding pair of electrons in a covalent bond

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12
Q

What happens it you increase the electronegativity?

A

Increases the electrons attracted to it

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13
Q

What are the three factors affecting electronegativity?

A

Atomic charge,distance from nucleus, electron shielding

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14
Q

How does electronegativity increase in the periodic table?

A

Across the groups and up the period

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15
Q

Would the dipole be negative or positive it the atom was more electronegative than the other?

A

Negative

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16
Q

What happens to the dipole is there is a greater difference of electronegarivity?

A

Greater permanent dipole

17
Q

What is a permanent dipole?

A

The charge difference between two bonded atoms of different electronegativities

18
Q

Are symmetrical bonds polar or non polar?

A

Non polar

19
Q

What are symmetrical molecules?

A

There are not just areas of just positive or just negative charge

20
Q

Which is the most electronegative element?

A

Fluorine

21
Q

What effect on polarity do lone pairs have?

A

Can cancel out dipoles created by bonding pairs

22
Q

What are intermolecular forces?

A

Weak interactions between dipoles of different molecules

23
Q

What are London forces? And what are they caused by?

A

Weak intermolecular forces caused by very small dipoles in molecules.

24
Q

What are factors affecting strength ?

A

The greater the number of electrons in each molecule,the larger the oscillating and induced dipoles and the greater the attractive forces between molecules

25
Q

What is a polar molecule?

A

A molecule which atoms have significant differences in their electronegativity and a dipole created

26
Q

What elements can hydrogen bonding occur?

A

Fluorine, nitrogen and oxygen

27
Q

What is hydrogen bonding?

A

Special type of dipole-dipole interaction

28
Q

Why does hydrogen only bond with specific atoms?

A

Hydrogen has a high density and F,N and O are highly electronegative

29
Q

What is the best example of hydrogen bonding?

A

Water

30
Q

What happens to water when it freezes?

A

The density decreases

31
Q

What is the structure of ice and what happens to it when it melts?

A

Diamond structure and it will collapse

32
Q

What happens to most simple molecular lattices (minus h20)?

A

They sublime, water doesn’t due to the hydrogen bonds

33
Q

What properties do water get from hydrogen bonds?

A

Relatively high viscosity and surface tension

34
Q

What happens to the surface tension on q liquid if you disrupt the hydrogen bonds?

A

It decreases