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chemistry gcse > 1chemical formulae, equations and calculations and ionic bonding > Flashcards

1chemical formulae, equations and calculations and ionic bonding Flashcards

1
Q

rfm =

A

ram (thing under the element on periodic table)

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2
Q

moles =

A

mass / rfm

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3
Q

percentage yield =

A

(actual yield / theoretical yield) x 100

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4
Q

molecular formula

A

the formula that shows the number and type of each atom in a molecule

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5
Q

empirical formula

A

the simplest whole number ratio of the atoms of each element present in one molecule or formula unit of the compound

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6
Q

organic molecules often have different

A

molecular and empirical formulas

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7
Q

the formula of an ionic compound is always

A

an empirical formula

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8
Q

empirical formula gives

A

the simplest whole number ratio of atoms of each element in the compound

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9
Q

an ion is

A

an electrically charged atom or group of atoms formed by the loss or gain of electrons

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10
Q

the loss or gain of electrons takes place to

A

obtain a full outer shell of electrons

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11
Q

negative ions are called

A

anions and form when atoms gain electrons- meaning they have more electrons than protons

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12
Q

positive ions are called

A

cations and form when atoms lose electrons- meaning they have more protons than electrons

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13
Q

all metals lose electrons to

A

become positively charged ions

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14
Q

all non metals gain electrons

A

from other atoms to become negatively charged ions

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15
Q

how do deduce the charge of an ion

A
  • Find the number of electrons in the outer electron shell
  • Find out if it is easy for the atom to gain electron or to donate electron (in most cases atoms that have fewer than four electrons, donate electrons and atoms that have more than 4 electrons, receive electrons)
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16
Q

atoms that gain electrons become

A

negatively charged and atoms that donate electrons form positive ions

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17
Q

charge/formula of group 1 metals

A

1+

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18
Q

charge/formula of group 2 metals

A

2+

19
Q

charge/formula of group 3 metals

A

3+

20
Q

charge/formula of silver

A

Ag+

21
Q

charge/formula of copper (II)

A

Cu2+

22
Q

charge/formula of iron (II)

A

Fe2+

23
Q

charge/formula of iron (III)

A

Fe3+

24
Q

charge/formula of lead

A

Pb2+

25
Q

charge/formula of zinc

A

Zn2+

26
Q

charge/formula of hydrogen

A

H+

27
Q

charge/formula of ammonium

A

NH+

4

28
Q

charge/formula of group 5 non metals

A

3-

29
Q

charge/formula of group 6 non metals

A

2-

30
Q

charge/formula of group 7 non metals

A

1-

31
Q

charge/formula of hydroxide

A

OH-

32
Q

charge/formula of carbonate

A

CO 2-

3

33
Q

charge/formula of nitrate

A

NO -

3

34
Q

charge/formula of sulphate

A

SO 2-

4

35
Q

charge/formula of chromium (III)

A

Cr 3+

36
Q

charge/formula of hydrogen carbonate

A

HCO -

3

37
Q

for ionic compounds you have to balance the charge of each part by

A

multiplying each ion until the sum = 0

38
Q

ionic bonding

A

the electrostatic force of attraction between oppositely charged ions

39
Q

ionic compounds are made up of

A

charged particles called ions which from a giant lattice structure

40
Q

ionic substances- mp/bp

A

ionic substances have high melting and boiling points due to the presence of strong electrostatic forces acting between the oppositely charged ions

41
Q

ionic compounds at room temp

A

usually solid and are non-volatile (do not vaporise easily)

42
Q

ionic compounds can conduct electricity in

A

molten state or in solution as they have ions that can move and carry charge

43
Q

why can’t ionic compounds conduct electricity in solids states

A

as the ions are in fixed positions within the lattice and are unable to move

chemistry gcse (21 decks)

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