3.2/3 ATOMIC STRUCTURE + IONIC BONDING Flashcards

1
Q

Define an isotope

A

Atoms of the same element, that have a different number of neutrons but same number or protons and electrons.

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2
Q

How do different isotopes affect the chemical and physical properties of an atom

A

It has the same chemical properties, but the melting point and density are different

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3
Q

What happens to the electrons in a metal ion

A

They lose electrons to give it a positive charge

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4
Q

What happens to the electrons in a non-metal ion

A

They gain electrons to give it a negative charge

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5
Q

What is reduction in ions

A

Gain of electrons

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6
Q

What is oxidation in ions

A

Loss of electrons

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7
Q

How do you calculate the relative atomic mass

A

1) Multiply the abundances by the mass and divide by 100
2) Do the same for all the isotopes.
3) Add them together

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8
Q

Define ionic bonding

A

The strong electrostatic attraction between oppositely charged ions

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9
Q

What are the relative masses and relative charges of the subatomic particles

A

Proton- 1
Neutron- 1
Electron- 0.001

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10
Q

What does the atomic number tell you about an atom

A

The number of protons

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11
Q

What does the mass number tell you about an atom

A

The number of protons and neutrons

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12
Q

What is a cross on a dot and cross diagram

A

The electrons the atom already has

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13
Q

What is a dot on a dot and cross diagram

A

The electrons it has gained

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14
Q

How do you draw a dot and cross diagram

A

1) Draw out all the atoms needed
2) Draw arrows from outer shell electrons from the metal to the outer shell electrons of the non-metal
3) Draw an arrow labeled ion on it
4) In brackets, draw the newly formed ions with the relevant electrons in crosses and dots with the charge outside the brackets in the top right corner and shell configuration on the bottom

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15
Q

How are ionic compounds arranged

A

A giant ionic lattice layered

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16
Q

Why do ionic compounds have high melting points

A

1) The ionic bonds are very strong
2) In a giant ionic lattice there are lots of ionic bonds
3) Breaking all the ionic bonds requires a large amount of energy

17
Q

How does the charge of ions in the giant ionic lattice affect the strength of the structure

A

The more charge in the ions, the stronger the giant ionic lattice

18
Q

Why aren’t solid ionic compounds conductors

A

The electrons aren’t free to move

19
Q

Why can ionic compounds conduct as a liquid

A

The electrons are free to move

20
Q

Why do ionic compounds conduct electricity when molten or dissolved but not solid

A

1) When solid, the ions are fixed and not free to move , so they cannot carry charge or flow
2) When they are dissolved or molten the ions are free to move allowing charge to flow therefore becoming conductive

21
Q

Are ionic substances soluble in water

A

Usally

22
Q

Describe the visual appearance of an ionic compound

A

Crystalline

23
Q

Are ionic substances brittle or malleable

A

Brittle