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BMAT Chemistry > ATOMS AND MOLECULES PT 2 > Flashcards

ATOMS AND MOLECULES PT 2 Flashcards

1
Q

how does an element become an ion

A

An element becomes an ion when it has more or fewer electrons than protons

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2
Q

what are anions

A

Negative ions

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3
Q

what are cations

A

Positive ions

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4
Q

A loss of electrons from a neutral atom creates what

A

cation

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5
Q

A gain of electrons from a neutral atom creates what

A

anion

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6
Q

what type of element tends to form a cation and an anion respective of each other

A

metals > cations

non-metals > anions

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7
Q

what happens to atomic size from right to left of periodic table

A

Atomic size (radius) increases

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8
Q

why does atomic size change from right to left of periodic table

A
  1. effective nuclear charge increases (more protons) from left to right
  2. each additional electron is pulled more strongly toward the nucleus
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9
Q

what happens to atomic size from top to bottom of periodic table

A

Atomic size (radius) increases

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10
Q

why does atomic size change from top to bottom of periodic table

A

the atom becomes larger with each added shell

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11
Q

Why does atomic radii increase from top to bottom

A

each underlying period will have elements with an extra shell of electrons

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12
Q

explain the trend of the periodic table in atomic radii using the two elements of helium and lithium from group 8

A

helium has one shell and lithium has two shells

shell increase cos extra period down

thus atomic radii increases from top to bottom of periodic table

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13
Q

what is Ionisation energy

A

energy required to remove an electron from an atom

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14
Q

what happens if en electron is closer to the nucleus of an atom in regards to ionisation energy

A

If an electron is more strongly attached to the nucleus, it requires more energy to be removed

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15
Q

how does ionisation change from left to right of the periodic table

A

increases

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16
Q

how does ionisation change from bottom to top of the periodic table

A

increases

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17
Q

why does ionisation energy increase when going from bottom to top of the periodic table [2 marks]

A
  1. increased distance creates a decrease in electric field strength
  2. thus less energy is required to remove an electron
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18
Q

what happens to distance of electrons when moving down the periodic table

A

distance of the electron from the nucleus increases because there are more electron shells when going down the periodic table

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19
Q

what happens to ionisation energy as you move up the periodic table

A

distance of the electron from the nucleus increases because there are more electron shells when going down the periodic table

increased distance creates a decrease in electric field strength and thus less energy is required to remove an electron

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20
Q

what is electronegativity

A

the tendency of an atom to attract an electron in a bond that it shares with another atom

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21
Q

what is the trend of electronegativity from left to right and down to up of periodic table

A

Electronegativity tends to increase from left to right and from bottom to top

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22
Q

what is the bond between atoms of the same molecule called

A

interactions between atoms within the molecule are known as intramolecular bonds

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23
Q

what is the bond between atoms of different molecule called

A

interactions between atoms in different molecules are known as intermolecular bonds

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24
Q

what are the three main intramolecular bonds within molecules

A

ionic
covalent
metallic

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25
Q

what are the three main IMF bonds

A

Van der Waals
Dipole-dipole
Hydrogen bonds

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26
Q

what does IMF stand for

A

intermolecular bond

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27
Q

When does a covalent bond occur

A

when two electrons are shared by two nuclei

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28
Q

What happens to the electrons within a covalent bond

A

electrons (negatively charged) are pulled toward both positively charged nuclei via electrostatic forces.

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29
Q

How are electrons pulled towards both nuclei in a covalent bond

A

via electrostatic forces

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30
Q

What is a hydrogen bond a special circumstance of

A

special case of dipole forces

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31
Q

What is a hydrogen bond

A

is the attractive force between the hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule

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32
Q

In a hydrogen bond, what element is the electronegative atom within the interaction bond usually

A

Usually the electronegative atom is nitrogen, fluorine, or oxygen

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33
Q

What does NFO all have in common

A

has a partial negative charge

34
Q

What happens to hydrogen when bonded to NFO

A

The hydrogen then has a partial positive charge as NFO all have a partial negative charge

35
Q

If hydrogen is bonded to atoms with slight negative charges, what charge will hydrogen have

A

positive charge

36
Q

What type of bond is an ionic bond

A

chemical bond

37
Q

What does an ionic bond involve

A

involves the electrostatic attraction between oppositely charged ions

38
Q

What is the primary bond that we observe from ionic compounds

A

ionic bonding

39
Q

What are van Der waals interactions

A

interaction of electron clouds between molecules

40
Q

What is the weakest intermolecular bond

A

van Der waals

41
Q

What is a hydrophobic interaction

A

interactions are intermolecular and occur between non-polar substances.

42
Q

What does hydrophobic bonds occur between

A

occur between non-polar substances.

43
Q

When is a compound formed

A

when a substance contains one or more elements in a definite ratio

44
Q

What is an example of an undeniable compound

A

water is a compound that contains oxygen and hydrogen in a definite ratio.

45
Q

What is empirical formula

A

simplest whole number ratio between the number of atoms of the different elements in the compound

46
Q

What is the formation of water as a symbol equation

A

2H2 + 02 > 2H20

47
Q

What is the empirical formula of benzene

A

CH

48
Q

What is the empirical formula of glucose

A

CH20

49
Q

What is the MF of benzene

A

C6H6

50
Q

What is the MF of glucose

A

C6 H12 06

51
Q

What is the MF of butane

A

c4 h10

52
Q

What is MF

A

the exact number of the different atoms that make up the molecule

53
Q

What are ionic compounds named after

A

named after their cation and anion

54
Q

When naming an ionic compound, how is the name positioning arranged

A

cation first

anion second

55
Q

What are monoatomic and polyatomic ions given the name suffix of

A

-ide

56
Q

In sodium chloride, which is the cation and which is the anion

A 
Na+ = cation
Cl- = anion
57
Q

What do hydrochloric acid and sodium form to make

A

sodium chloride

58
Q

What’s the symbol equation for the combination of Cl and Na

A

2Na + Cl2 > 2NACl

59
Q

What is the law of conservation of mass

A

the number of atoms of a given element remains constant during the process of a chemical reaction

60
Q

What are the four fundamental types of reactions

A

combination
decomposition
single displacement
double displacement

61
Q

What is a single displacement represented in symbols

A

A + BC > B + AC

62
Q

What is a double displacement represented in symbols

A

AB + CD > AD + BC

63
Q

What is a synthesis reaction

A

where two or more elements chemically combine to give a compound

64
Q

What is a decomposition reaction

A

compound if broken down to simple elements

65
Q

What is a substitution reaction

A

an atom of group is replaced by another atom or group

66
Q

What is a precipitation reaction

A

where a solid compound is formed when solutions of two soluble compounds are mixed

67
Q

What is a neutralisation reaction

A

reactions where acid reacts with a base to give salt and water

68
Q

What is a redox reaction

A

where electron transfer occurs

69
Q

What does oxidised and reduced mean in terms of oxidation state

A

change in oxidation state

oxidised = increased oxidation state

reduced = decreased oxidation state

70
Q

The oxidation number for an element can be calculated how

A

always 0

71
Q

What is the oxidation number of a monoatomic ion

A

charge of the monoatomic ion

72
Q

What is the oxidation number of all group 1 metals

A

+!

73
Q

What is the oxidation number of all group 2 metals

A

+2

74
Q

What is the oxidation number of Hydrogen

A

+1 when bonded to a nonmetal

-1 when bonded to a metal.

75
Q

What is the oxidation number of Oxygen

A
  • 1 in peroxides (O22-)—uncommon

- 2 in all other compounds—most common.

76
Q

What is the oxidation number of fluorine

A

-1

77
Q

What is the oxidation state of a poly atomic ion

A

charge on the polyatomic ion

78
Q

What is an oxidising agent

A

agent will cause oxidation to occur, whilst the agent itself will be reduced.

79
Q

What is a reducing agent

A

agent will cause reduction to occur, whilst the agent itself will be oxidised.

80
Q

What happens when something is reduced

A

gains electrons.

81
Q

What happens when something is oxidised

A

it loses electrons.

82
Q

what is the sum of the oxidation numbers of all atoms in a neutral compound

A

0

BMAT Chemistry (7 decks)

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