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Steps2Success > Bonding > Flashcards

Bonding Flashcards

1
Q

What is ionic bonding?

A

bonding where an electron is added/lost, changing the charges of the atoms and creating electrostatic forces of attraction

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2
Q

how do elements react?

A

by ensuring they have a complete outer shell

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3
Q

what are the attractions between two opposite charged ions called?

A

electrostatic forces of attractions

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4
Q

Why do ionic compounds have high melting and boiling points?

A

because they have strong electrostatic attractions that require a high amount of energy to break

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5
Q

when do ionic compounds conduct electricity?

A

when they are molten or dissolved

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6
Q

why don’t ionic compounds conduct electricity when solid?

A

because the ions are not free to carry the charge

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7
Q

why can ionic compounds conduct electricity when molten/dissolved?

A

because the ions are free to move, meaning they can carry the charge

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8
Q

What is covalent bonding?

A

bonding where the two metals/non-metals share elctrons to complete the outer shell

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9
Q

give two examples of covalent bonding

A

diamond and graphite

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10
Q

how many bonds are formed from one atom in diamond covalent bonding?

A

4 from each atom

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11
Q

why does diamond covalent bonding not conduct electricity?

A

there are no free electrons to carry the charge

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12
Q

how many covalent bonds form from one atom in graphite bonding?

A

three covalent bonds

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13
Q

why does graphite conduct electricity?

A

there is a delocalised electron to carry the charge

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14
Q

why is graphite structure usually soft and slippery?

A

because there are weak intermolecular forces between the layers

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15
Q

why is there a high melting point and boiling point on diamond and graphite covalent bonding?

A

because the bonds between atoms are strong and take a large amount of energy to break

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16
Q

when do metal atoms become positively charged?

A

when they lose an electron

17
Q

what is metallic bonding?

A

bonds between the delocalised electrons and positively charged atoms in metals

18
Q

why are metals able to conduct electricity?

A

because the delocalised electrons are free to move through the structure

19
Q

why do metals have high melting/boiling point?

A

because the electrostatic bonds between the electrons and ions are strong and take a large amount of energy to break

20
Q

why can metals slide over each other and can be bent/shaped?

A

because the layers can slide over each other due to the delocalised electrons

Steps2Success (6 decks)

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