Structure and bonding Flashcards

1
Q

What is electronegativity?

A

The ability of an atom to attract electrons towards itself in a covalent bond

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2
Q

The further up and right you go in the periodic table, the more…

A

Electronegative an element is

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3
Q

What is the most electronegative element on the periodic table?

A

Fluorine

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4
Q

What scale helps to identify how electronegative an element is?

A

The Pauling Scale

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5
Q

If there’s a big difference in electronegativity in a compound, what does this mean?

A

The compound will be more ionic and the bond will be more polar

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6
Q

If there’s an electronegative difference of 0, what does this tell us about the molecule?

A

That it’s mostly covalent

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7
Q

What’s an example of a mostly covalent molecule?

A

Cl2

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8
Q

Are hydrocarbons polar or non polar?

A

Non polar

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9
Q

Why is carbon dioxide non polar?

A

Because the polar bonds are arranged symmetrically and so overall there’s no polarity

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10
Q

What is the strongest intermolecular force?

A

Hydrogen bonds

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11
Q

What is the weakest intermolecular force?

A

London forces

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12
Q

What molecules or atoms do London forces exist in?

A

All molecules and atoms with electrons

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13
Q

Are more London forces existent in molecules/atoms that are bigger?

A

Yes because larger molecules/atoms have more electrons

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14
Q

Which hydrocarbons have more London forces?

A

Longer, straight chained hydrocarbons

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15
Q

Why do branched hydrocarbons have less London forces?

A

Because they can’t pack together as close

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16
Q

What atoms/molecules are permanent dipole-dipole interactions existent in?

A

Atoms/ molecules with a polarity

17
Q

Which has weaker London forces, alkanes or alcohols?

A

Alkanes

18
Q

Do halides have permanent dipoles?

A

Yes

19
Q

What are the 3 most electronegative elements on the periodic table?

A

Nitrogen, oxygen, and fluorine

20
Q

What needs to be present for hydrogen bonding to occur?

A

Hydrogen bonded to a strongly electronegative element and at least 1 lone pair of electrons

21
Q

What must happen in order for a substance to dissolve?

A

The substance’s bonds must break, the solvent’s bonds must break, and new bonds must form between the substance and the solvent.

22
Q

Do alcohols dissolve in polar solvents?

A

Yes, because they can hydrogen bond with water molecules.

23
Q

Why can’t the hydrocarbon part of an alcohol dissolve in water?

A

Because the hydrocarbon part is non polar and so doesn’t dissolve in water

24
Q

How does the size of an alcohol affect its solubility?

A

The bigger the hydrocarbon part, the less soluble the alcohol is

25
Q

Why do some polar molecules, like haloalkanes, not dissolve in water?

A

Because their dipoles aren’t very strong and water molecules can form stronger hydrogen bonds with each other.

26
Q

What type of solvents can haloalkanes dissolve in?

A

Solvents that interact via permanent dipole-dipole interactions

27
Q

Are alkanes polar or non polar?

A

They’re non polar and they dissolve best in non polar solvents as they can form London forces between the molecules

28
Q

What is the polarising power as applied to cations?

A

The ability of a cation to change the shape of an electron cloud around an anion

29
Q

What is the strongest intermolecular force in methane?

A

London forces

30
Q

What’s the strongest intermolecular force in Hydrogen Fluoride?

A

Hydrogen bonding

31
Q

If the bond polarities don’t cancel then a molecule is what?

A

Polar

32
Q

How can you distinguish between solid lithium chloride and solid sodium chloride?

A

-Put nichrome wire in solid and place in hot/blue flame
-The lithium salt should give a chrimson colour
-The sodium salt should give a yellow colour

33
Q

What are London forces or Van Der Waals forces caused by?

A

They’re caused by the asymmetry of the electron cloud, hence causing attractive forces between neighbouring dipoles