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BMAT Chemistry > ATOMS AND MOLECULES PT 2 > Flashcards

ATOMS AND MOLECULES PT 2 Flashcards

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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
what are the three main IMF bonds
Van der Waals Dipole-dipole Hydrogen bonds
26
what does IMF stand for
intermolecular bond
27
When does a covalent bond occur
when two electrons are shared by two nuclei
28
What happens to the electrons within a covalent bond
electrons (negatively charged) are pulled toward both positively charged nuclei via electrostatic forces.
29
How are electrons pulled towards both nuclei in a covalent bond
via electrostatic forces
30
What is a hydrogen bond a special circumstance of
special case of dipole forces
31
What is a hydrogen bond
is the attractive force between the hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule
32
In a hydrogen bond, what element is the electronegative atom within the interaction bond usually
Usually the electronegative atom is nitrogen, fluorine, or oxygen
33
What does NFO all have in common
has a partial negative charge
34
What happens to hydrogen when bonded to NFO
The hydrogen then has a partial positive charge as NFO all have a partial negative charge
35
If hydrogen is bonded to atoms with slight negative charges, what charge will hydrogen have
positive charge
36
What type of bond is an ionic bond
chemical bond
37
What does an ionic bond involve
involves the electrostatic attraction between oppositely charged ions
38
What is the primary bond that we observe from ionic compounds
ionic bonding
39
What are van Der waals interactions
interaction of electron clouds between molecules
40
What is the weakest intermolecular bond
van Der waals
41
What is a hydrophobic interaction
interactions are intermolecular and occur between non-polar substances.
42
What does hydrophobic bonds occur between
occur between non-polar substances.
43
When is a compound formed
when a substance contains one or more elements in a definite ratio
44
What is an example of an undeniable compound
water is a compound that contains oxygen and hydrogen in a definite ratio.
45
What is empirical formula
simplest whole number ratio between the number of atoms of the different elements in the compound
46
What is the formation of water as a symbol equation
2H2 + 02 > 2H20
47
What is the empirical formula of benzene
CH
48
What is the empirical formula of glucose
CH20
49
What is the MF of benzene
C6H6
50
What is the MF of glucose
C6 H12 06
51
What is the MF of butane
c4 h10
52
What is MF
the exact number of the different atoms that make up the molecule
53
What are ionic compounds named after
named after their cation and anion
54
When naming an ionic compound, how is the name positioning arranged
cation first | anion second
55
What are monoatomic and polyatomic ions given the name suffix of
-ide
56
In sodium chloride, which is the cation and which is the anion
``` Na+ = cation Cl- = anion ```
57
What do hydrochloric acid and sodium form to make
sodium chloride
58
What’s the symbol equation for the combination of Cl and Na
2Na + Cl2 > 2NACl
59
What is the law of conservation of mass
the number of atoms of a given element remains constant during the process of a chemical reaction
60
What are the four fundamental types of reactions
combination decomposition single displacement double displacement
61
What is a single displacement represented in symbols
A + BC > B + AC
62
What is a double displacement represented in symbols
AB + CD > AD + BC
63
What is a synthesis reaction
where two or more elements chemically combine to give a compound
64
What is a decomposition reaction
compound if broken down to simple elements
65
What is a substitution reaction
an atom of group is replaced by another atom or group
66
What is a precipitation reaction
where a solid compound is formed when solutions of two soluble compounds are mixed
67
What is a neutralisation reaction
reactions where acid reacts with a base to give salt and water
68
What is a redox reaction
where electron transfer occurs
69
What does oxidised and reduced mean in terms of oxidation state
change in oxidation state oxidised = increased oxidation state reduced = decreased oxidation state
70
The oxidation number for an element can be calculated how
always 0
71
What is the oxidation number of a monoatomic ion
charge of the monoatomic ion
72
What is the oxidation number of all group 1 metals
+!
73
What is the oxidation number of all group 2 metals
+2
74
What is the oxidation number of Hydrogen
+1 when bonded to a nonmetal | -1 when bonded to a metal.
75
What is the oxidation number of Oxygen
- 1 in peroxides (O22-)—uncommon | - 2 in all other compounds—most common.
76
What is the oxidation number of fluorine
-1
77
What is the oxidation state of a poly atomic ion
charge on the polyatomic ion
78
What is an oxidising agent
agent will cause oxidation to occur, whilst the agent itself will be reduced.
79
What is a reducing agent
agent will cause reduction to occur, whilst the agent itself will be oxidised.
80
What happens when something is reduced
gains electrons.
81
What happens when something is oxidised
it loses electrons.
82
what is the sum of the oxidation numbers of all atoms in a neutral compound
0

BMAT Chemistry (7 decks)

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