U1-3-1 - Bond Polarity Flashcards

Part of the Structure and Bonding topic from Unit 1 of Higher Chemistry, Chemical Changes and Structure

1
Q

Formula for phosphorus

A

P4

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2
Q

Formula for sulfur

A

S8

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3
Q

Name all covalent network elements

A

Boron, silicon, carbon

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4
Q

Pure covalent bond

A

A bond in which bonding electrons are shared equally.

Also called ‘non-polar bond’

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5
Q

Polar bond

A

A bond in which bonding electrons are shared unequally and which has a permanent dipole.

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6
Q

What causes chemical bonds to be polar?

A

Electronegativity difference between bonding atoms.

(usually ≥0.4)

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7
Q

How do you determine the ‘ionic character’ of a bond?

A

Calculate electronegativity difference.

Higher ΔEN = more ionic character (bonding e- shared less evenly)

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8
Q

What do δ+ and δ− mean?

A

Delta plus/delta minus - partial charges

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9
Q

A compound has a low melting/boiling point and does not conduct electricity in any form.

What bonding and structure does it have?

A

Covalent molecular

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10
Q

A compound has a very high melting/boiling point and does not conduct electricity in any form.

What bonding and structure does it have?

A

Covalent network

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11
Q

A compound has a very high melting/boiling point and conducts electricity when molten/dissolved.

What bonding and structure does it have?

A

Ionic (lattice)

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12
Q

Li+2S2−

What is wrong with this ionic formula?

A

More than one of Li+ present, must be shown in brackets:

(Li+)2S2−

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