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Chemistry GCSE > 2 Periodic Table + Bonding > Flashcards

2 Periodic Table + Bonding Flashcards

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1
Q

What is the reactivity series of metals?

A 
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
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2
Q

What happens in ionic bonding?

A

Atoms lose or gain electrons to form charged particles called ions.

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3
Q

Why are ions strongly attracted to one another?

A

Because they have opposite charges.

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4
Q

What do we call it when ions are strongly attracted to one another?

A

Electrostatic attraction

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5
Q

What does Electrostatic attraction cause?

A

High melting + Boiling points.

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6
Q

What groups lose electrons easily?

A

1 ,2 and 6, 7

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7
Q

What do electrons in group 1 and 2 want to do?

A

Lose

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8
Q

What do electrons in group 6 and 7 want to do?

A

Gain

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9
Q

What is an Isotope?

A

Same number of protons + electrons, different number of neutrons.

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10
Q

Do regular atoms and isotopes react the same or differently and why?

A

Same - same number of electrons.

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11
Q

Do regular atoms and ions react the same or differently and why?

A

Differently - different number of electrons.

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12
Q

What is an atom?

A

Smallest particle of an element that still has chemicals properties of an element.

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13
Q

What are atoms made of?

A

Smaller sub-atomic particles.

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14
Q

What is the same about all atoms of an element?

A

All equally charged.

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15
Q

What are the three subatomic particles, what are their features and where are they found?

A 
Proton = Positive, in nucleus
Electron = Negative, along shells
Neutrons = Neutral, in nucleus.
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16
Q

What are the masses of each of the sub atomic particles?

A 
Proton = 1
Electron = 1
Neutron = 1/1836
17
Q

Write the electron configuration of carbon? (6 electrons)

A

2, 4

18
Q

What are the physical properties of simple covalent molecules and why?

A

Low B.PT. = Weak intermolecular forces of attraction

Don’t conduct electricity = don’t have freely moving charge carriers.

19
Q

What happens if the molecular mass increases of a simple covalent molecule?

A

number of weak intermolecular forces also increase, so more heat required to break so higher M.PT.

20
Q

What is a covalent bond?

A

Shared electron pair?

21
Q

Draw a dot and cross diagram for hydrogen (like on a piece of paper, like now then check online)

A

Did you get it right?

22
Q

Draw a dot and cross diagram for CH4 (like on a piece of paper, like now then check online)

A

Did you get it right?

23
Q

Why do covalent bonds exist?

A

Because of the electrostatic attraction between the negative electrons and the positive nucleus.

24
Q

What is a giant covalent structure?

A

Large molecules made up of many atoms.

25
Q

Giant covalent structures are allotropes, what does that mean?

A

Made up of the same element.

26
Q

What are the properties of diamond? /3

A
  1. Is a giant covalent structure.
  2. Each carbon atom forms 4 strong covalent bonds so had no freely moving charge carriers to conduct electricity
  3. Melting point is high because lots of heat energy needs to break strong covalent bonds
27
Q

What are the properties of graphite? /5

A
  1. Is a giant covalent structure.
  2. Each carbon atom forms 3 strong covalent bonds and 1 weak intermolecular force,
  3. has one freely moving charge carriers for each bond to conduct electricity.
  4. High M.PT. because it has many strong covalent bonds.
  5. Is in layers
28
Q

What are the properties of C-60 Fullerene? /3

A
  1. Low M.PT. weak intermolecular forces - don’t need much energy to break
  2. Have ability to conduct electricity because one bond is free.
  3. Only 3 strong covalent bonds.
29
Q

Why is graphite a lubricant?

A

Layers can slide easily

Weak intermolecular forces - easy to break

Chemistry GCSE (12 decks)

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