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Chemistry > Bonding and Structure > Flashcards

Bonding and Structure Flashcards

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1
Q

how do you know the number of protons in an atom?

A

atomic number

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2
Q

how do you know the number of neutrons in an atom?

A

mass number - atomic number

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3
Q

how do you know the number of electrons in an atom?

A

atomic number

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4
Q

what is the charge for group 1 elements?

A

+1

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5
Q

what is the charge for group 2 elements?

A

+2

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6
Q

what is the charge for group 3 elements?

A

+3

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7
Q

what is the charge for group 5 elements?

A

-3

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8
Q

what is the charge for group 6 elements?

A

-2

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9
Q

what is the charge for group 7 elements?

A

-1

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10
Q

what is the ion for silver?

A

Ag+

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11
Q

what is the ion for copper?

A

Cu²+

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12
Q

what is the ion for iron?

A

Fe²+ / Fe³+

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13
Q

what is the ion for lead?

A

Pb²+

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14
Q

what is the ion for zinc?

A

Zn²+

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15
Q

what is an anion?

A

a negative ion

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16
Q

what is a cation?

A

a positive ion

17
Q

why do ions have high melting and boiling points?

A

strong electrostatic forces of attraction which require lots of energy to overcome

18
Q

how are ions formed?

A

when a metal and non-metal reacts

19
Q

why can ions conduct electricity when dissolved or molten?

A

the ions are free to move and can carry a charge

20
Q

why can’t ions conduct electricity as solids?

A

the ions are not free to move

21
Q

how is a covalent bond formed?

A

when atoms (usually 2 non-metals) share pairs of electrons

22
Q

why do compounds with giant ionic lattices have high melting and boiling points?

A

strong electrostatic forces of attraction which require lots of energy to overcome

23
Q

why do simple molecular compounds have low melting and boiling points?

A

weak intermolecular forces of attraction which require little amount of energy to overcome

24
Q

why do giant covalent structures (like diamond and graphite) have such high melting and boiling points?

A

strong covalent bonds which require a lot of energy to overcome

25
Q

can diamond conduct electricity? and why?

A

no diamond is an insulator because it has no delocalised electrons

26
Q

can graphite conduct electricity? and why?

A

yes graphite is a conductor because it has delocalised electrons which can carry a charge through the structure

27
Q

can buckminsterfullerene’s conduct electricity? and why?

A

no C60 is an insulator because although it has delocalised electrons, these electrons cannot move from molecule to another

28
Q

what is the strength of diamond?

A

very strong and hard

29
Q

what is the strength of graphite?

A

soft and brittle

30
Q

what is the strength of C60?

A

soft

31
Q

why do covalent compounds not conduct electricity

A

because they are neutral and there are no charged particles (ions) to move and carry a charge

32
Q

what is an alloy?

A

a mixture of a metal and one or more elements - usually other metals or carbon

33
Q

what is an allotrope?

A

different forms of the same element (for example C60, diamond and graphite are 3 allotropes of carbon)

34
Q

how can metals conduct electricity?

A

they have delocalised electrons that can carry a charge and move around the metal ions

35
Q

true or false? metals are malleable. if so why?

A

true. metals can be hammered into thin sheets without breaking. this is due to the electrostatic attractions within the structure

36
Q

why are alloys stronger than pure metals?

A

because they contain atoms of different sizes which distorts the regular arrangements of atoms. this makes it more difficult for the layers to slide over each other

37
Q

what are the electrostatic attractions of metallic bonding?

A

strong electrostatic attraction between sea of negative delocalised electrons and positive metal ions

38
Q

what is a compound?

A

2 or more different elements chemically bonded together

Chemistry (3 decks)

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