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Grade 8 Science > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

In ionic bonding, what happens to the electrons

A

The electrons are transferred

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2
Q

In covalent bonding, what happens to the electrons

A

The electrons are shared

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3
Q

In ionic bonding, what is it between

A

Metal and non-metal

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4
Q

In covalent bonding, what is it between

A

Non-metals

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5
Q

In ionic bonding, what force holds it together (2)

A

Electrostatic force of attraction between oppositely charged ions (positive and negative)

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6
Q

Definition of compound (2)

A

DIFFERENT elements JOINED together

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7
Q

In covalent bonding, what happens to the electrons

A

The electrons are shared

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8
Q

In ionic bonding, what happens to the electrons

A

The electrons are transferred

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9
Q

In ionic bonding, what happens to the metal

A

Metal loses electrons to form a positive ion

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10
Q

In ionic bonding, what happens to the non-metal

A

Non-metals gain electrons to form negative ions

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11
Q

Ionic - description of melting point, and explanation (1+2)

A

High melting point
Strong electrostatic force of attraction that requires a lot of energy to break

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12
Q

Ionic - description of conductivity, and explanation (1+1)

A

Only conducts when molten or aqueous
The ions (charges) are free to move

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13
Q

Define molten

A

melted

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14
Q

Define aqueous

A

dissolved in solution

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15
Q

Simple covalent structure

A

Small molecule

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16
Q

How is simple covalent held together (2 - between atoms, between molecules)

A

Strong covalent bonds between atoms
Weak intermolecular forces between molecules

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17
Q

Simple covalent - description of melting point, and explanation (1+2)

A

Low melting point
It doesn’t require much energy to break the weak intermolecular forces

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18
Q

Simple covalent - description of conductivity, and explanation (1+1)

A

Does not conduct
There are no charged particles

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19
Q

Giant covalent structure

A

Giant lattice

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20
Q

How is giant covalent held together

A

Lots of strong covalent bonds

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21
Q

Giant covalent - description of melting point, and explanation (1+2)

A

High melting point
Requires a lot of energy to break the covalent bonds

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22
Q

Giant covalent - description of conductivity, and explanation (1+2)

A

Does not conduct except graphite
No free electrons except in graphite

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23
Q

Metallic structure (2)

A

Positive metal ions in a ‘sea’ of delocalised electrons

24
Q

Hot metallic is held together

A

Electrostatic force of attraction

25
Q

Metallic - description of melting point, and explanation (1+2)

A

High melting point
Strong electrostatic force of attraction that requires a lot of energy to break

26
Q

Metallic - description of conductivity (1+1)

A

Yes, they conduct
The electrons (charges) can move

27
Q

atomic number

A

the number of protons and electrons in an atom

28
Q

Lithium reaction with water: description, word equation, symbol equation

A

When lithium reacts with water, it sizzles and forms an alkaline solution - Lithium hydroxide
Lithium + water > Lithium hydroxide + hydrogen
2Li + H2O > H2 + 2LiOH

29
Q

Sodium reaction with water: description, word equation, symbol equation

A

When sodium reacts with water, it reacts more vigorously than lithium and forms an alkaline solution - Sodium hydroxide
Sodium + water > Sodium hydroxide + hydrogen
2Na + H2O > H2 + 2NaOH

30
Q

How do you calculate mass number

A

protons+neutrons

31
Q

mass and charge of electron

A

Mass = 1/2000
Charge = negative

32
Q

Mass and charge of neutron

A

Mass = 1
Charge = neutral

33
Q

Mass number

A

The number of protons and neutrons combined

34
Q

Mass and charge of proton

A

mass = 1
charge = +

35
Q

maximum electrons in the 1st shell

A

2

36
Q

maximum electrons in the 2nd shell

A

8

37
Q

maximum electrons in the 3rd shell

A

8

38
Q

Potassium reaction with water: description, word equation, symbol equation

A

When potassium reacts with water, it reacts more vigorously than sodium, burns with a lilac flame, produces a small popping noise, and forms an alkaline solution - Potassium hydroxide
Potassium + water > Potassium hydroxide + hydrogen
2K + H2O > H2 + 2KOH

39
Q

Trend in reactivity in group 1

A

Reactivity gets more vigorous as you go down the group

40
Q

Trends in boiling/melting points in group 0 (noble gases)

A

They increase

41
Q

Trends in boiling/melting points in group 1 (alkali metals)

A

They decrease

42
Q

Trends in boiling/melting points in group 7 (halogens)

A

They increase

43
Q

Sodium chloride what type of bond

A

ionic bond

44
Q

Sodium chloride structure

A

giant ionic lattice

45
Q

What holds sodium chloride together

A

electrostatic force of attraction holds the ions together

46
Q

Explain why iodine has a low melting point(2)

A

Weak intermolecular forces that do not require a lot of energy to break
Is a simple covalent (not giant covalent)

47
Q

Explain, in terms of particles, why liquid iodine does not conduct electricity (2)

A

There are no free electrons so
cannot carry charge through the structure

48
Q

Describe and explain giant ionic melting point (3)

A

high melting point
because strong electrostatic force of attraction that holds the ions together
that requires a lot of energy to break

49
Q

Describe and explain simple covalent melting point (3)

A

low melting point
because weak intermolecular forces of attraction between molecules
that do not require a lot of energy to break

50
Q

Describe and explain giant metallic melting point (3)

A

high melting point
because strong electrostatic force of attraction that holds the ions together
that requires a lot of energy to break

51
Q

Describe and explain giant covalent melting point (3)

A

high melting point
because strong covalent bonds between non-metals
that require a lot of energy to break

52
Q

Describe and explain if giant ionic conducts (3)

A

only conducts when molten or aqueous
because the ions (charges) are
free to move

53
Q

Describe and explain if simple covalent conducts (3)

A

Does not conduct
because there are no charged particles

54
Q

Describe and explain if giant metallic conducts (3)

A

Does conduct
because the delocalised electrons (charges)
can move

55
Q

Describe and explain if giant covalent conducts (3)

A

Does not conduct EXCEPT for graphite
because there are no free electrons
except for in graphite, there are

Grade 8 Science (7 decks)

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