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Chemistry > Reactivity + Ions + Chemical fomulae > Flashcards

Reactivity + Ions + Chemical fomulae Flashcards

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1
Q

What do atoms contain

A
  • protons
  • neutrons
  • electrons
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2
Q

What is the relative mass of a proton

A

1

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3
Q

What is the relative mass of a neutron

A

1

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4
Q

What is the relative mass of an electron

A

0.0005

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5
Q

What is the relative charge of a proton

A

+1

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6
Q

What is the relative charge of a neutron

A

0

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7
Q

What is the relative charge of an electron

A

-1

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8
Q

Where is the nucleus in the atom

A

in the middle

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9
Q

What does the nucleus contain

A

protons and neutrons

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10
Q

What is the charge of the nuclues

A

positive - because of the protons

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11
Q

Where do you find the electrons in an atom

A

in energy levels called shells moving around the nucleus

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12
Q

How do the number of protons and electron relate in a nutral atom

A

The number of electrons and protons are the same in a nutral atom

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13
Q

Why do neutral atoms have no charge

A

Because the number of negative electrons and positive protons cancel out

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14
Q

What happens to an atom if electrons are added or moved

A

the atom become charged and is now an ion

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15
Q

What does the atomic number tell you about an atom

A

How many protons there are

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16
Q

What does the mass number tell you about the atom

A

How many protons and neutrons are present in the atom in total

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17
Q

What are molecules

A

Groups of atoms

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18
Q

What is an isotope

A

Isotopes are different atomic forms of the same element, which have the same number of protons but different number of neutrons

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19
Q

What is relative atomic mass

A

The average mass of all the isotopes of an element

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20
Q

How do you work out the relative atomic mass

A

((mass number x percentage) of isotope 1 + (mass number x percentage) of isotope 2) / 100

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21
Q

What are ions

A

charged atoms

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22
Q

what do you call negative ions

A

anions

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23
Q

what do you call positive ions

A

cations

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24
Q

What does the charge of an ion depend on

A

How many electrons lost or gained

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25
Q

If an atom has lost electrons what will its charge be

A

positive

26
Q

If an atom has gained electrons what will its charge be

A

negative

27
Q

How can you find out the group number of an element

A

From the number of electrons on the outer shell

28
Q

How can you find out the period number of an element

A

From the number of occupied shells

29
Q

Why are the noble gases (group 0) so unreactive

A

Because they’re outer shell is already full - they’re already stable

30
Q

What groups lose electrons

A

groups:
- 1
- 2
- 3

31
Q

what groups gain electrons

A

groups:
- 5
- 6
- 7

32
Q

Explain what happens when elements react

A

When metals and non-metals react electrons from the metal element will be transferred to the non-metal element so that both elements become stable with a full outer shell

33
Q

What does the transfer of electron produce

A

An ionic compound

34
Q

What is an ionc bond

A

When the oppositely charged ions (metal and non-metal) are strongly attracted to one another by electrostatic attractions

35
Q

What is the formula for hydroxide

A

OH -

36
Q

What is the formula for Sulfate

A

SO4 2-

37
Q

What is the formula for carbonate

A

CO3 2-

38
Q

What is the formula for chloride

A

Cl -

39
Q

What is the formula for oxide

A

O 2-

40
Q

What happens to the charges in an ionic compound

A

The overall charge is zero so the negative charges in the compound must balance out the positive charges

41
Q

How would you work out the formula for an ionic compound

A

Write out both of the original formulas for the two elements and then figure out the ratio that gives an overall natural charge

42
Q

How would you show and ionic compound

A

Using a ‘dot and cross’ diagram

43
Q

What do you always need to put on a ‘dot and cross’ diagram

A
  • Brackets around the ions
  • The charge of each ion outside of the brackets
44
Q

What are two properties of ionic compounds

A
  • high melting point
  • high boiling point
45
Q

Are ionic compounds electrical conductors when solid

A

no

46
Q

How do you make ionic compounds electrical conductors

A

By melting them or dissolving them in water

47
Q

What structure do ionic compounds have

A

A lattice structure

48
Q

Why do ionic compounds have high boiling and melting points

A

Because a lot of energy is needed to overcome the strong attraction from the oppositely charged ions

49
Q

Describe the structure of ionic compounds

A

Ionic compounds are help together in a closely packed 3D lattice arrangement by the attraction between the oppositely charged ions

50
Q

what do equations show

A

The reactants and products of a reaction

51
Q

What is the state symbol for solid

A

(s)

52
Q

What is the state symbol for liquid

A

(l)

53
Q

What is the state symbol for gas

A

(g)

54
Q

What is the state symbol for aqueous (dissolved in water)

A

(aq)

55
Q

what do you do to balance an equation

A

By placing numbers in front of the formulas where needed

56
Q

how do you balance an equation

A

By ensuring that there are the same number of atoms of each element on both sides of the equation

57
Q

What are group 1 elements called

A

the alkali metals

58
Q

What is the basic equation for an alkali metal and water

A

metal + water -> metal hydroxide + hydrogen
2 + 2h2O(l) -> 2[]OH(aq) + h2(g)

59
Q

What happens to the reactivity as you go down the alkali metals

A

It increases - the metals become more reactive as you go down

60
Q

Why are alkali metals more reactive as you go down the group

A

Because the outermost electron is on a shell that’s further away from the nucleus so the electron is more easily lost

61
Q

Describe the process of ionic bonding

A

Ionic bonding is when a metal and a non-metal react together - transferring electrons . A metal atom loses its electron(s) to form a positive ion (cation) and a non-metal atom gains electron(s) to form a negative ion (anion). The bond is caused by the strong electrostatic attraction from the oppositely charged ion

Chemistry (15 decks)

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