Ionic, Covalent and Metallic bonding Flashcards

1
Q

What is a covalent bond ?

A

the attraction between the bonding pair of electrons and (2+) atomic nuclei

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2
Q

Why do metals conduct electricity ?

A

delocalised electrons, free to move from one side to the other. Thus conduct electricity. (flow of electrons)

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3
Q

Why are metals malleable ?

A

Layers can slide, when they do the positive metal ions are in the same environment as they were, still electrostatic attraction.

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4
Q

How does a Ionic bond differ to covalent ?

A

Ionic=m/nm covalent= nm/nm covalent=share electrons (no ions) ionic is opposite. (accept any other relevant answers)

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5
Q

Why are ionic compounds brittle ?

A

when force is applied, a cation may rearrange and be next to another cation=repulsion=brittle.

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6
Q

Name the attraction in a ionic lattice and why does it require so much energy to break up the lattice ?

A

electrostatic attraction, hard to overcome as it acts in all directions between anions and cations, requires lots of energy.

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7
Q

What is a dative bond and what does the arrow mean ?

A

is a covalent bond in which 1 molecule provides both pairs of electrons(lone pair), arrow=direction in which the electrons are given, from the donor.

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8
Q

Why can graphite conduct electricity and its layers slide ?

A

delocalised electrons and weak intermolecular forces between layers. (van der waal forces)

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9
Q

Place the following in order of strength; metallic, covalent and ionic.

A

1)covalent 2) ionic 3) metallic

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10
Q

name the types of crystal

A

molecular, ionic, covalent, metallic

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11
Q

of the 4(crystals) which is iodine, and why is little energy needed to break its structure ?

A

molecular: weak van der waal forces between molecules

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12
Q

what does crystalline and amorphous mean ?

A

crystalline= regular/neat fixed arranged pattern. Amorphous= no regular pattern

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13
Q

what is the electrostatic attraction between in a covalent bond ?

A

nuclei of atoms and bonding pair of electrons

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14
Q

why do no ions form ?

A

only involves sharing of electrons

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15
Q

give an example of a giant covalent structure + why high melting point

A

diamond: 4x covalent bond per C, giant covalent, lots of energy required

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