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Chemistry Unit 1 AS > Definitions > Flashcards

Definitions Flashcards

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0
Q

Ionic bond

A

the electrostatic attraction between positive ions and negative ions

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1
Q

Relative Isotopic Mass

A

the mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12

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2
Q

Salt

A

ionic compound formed from an acid when a H+ ion from acid had been replaced by a metal ion or another positive ion

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3
Q

Isotopes

A

atoms of the same element with the same number of protons but different numbers of neutrons and so different masses

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4
Q

relative atomic mass

A

the weighted mean mass of an atom of an element compared to one-twelfth of the mass of an atom of carbon-12

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5
Q

Avogadro’s constant

A

the number of atoms/particles per mole of a substance (of the carbon-12 isotope)
6.02 x10*23

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6
Q

relative molecular mass

A

weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12

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7
Q

mole

A

the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope

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8
Q

relative formula mass

A

weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12

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9
Q

molar mass

A

the mass per mole of a substance - gmol-1

can find it by adding all RAMs for each atom in the formula

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10
Q

avogadros hypothesis

A

equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

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11
Q

molar volume

A

volume per mole of gas molecules - dm3mol-1

at RTP molar vol is approx 24.0dm3mol-1

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12
Q

concentration of a solution

A

the amount of solute, in mol, dissolved per 1dm3 of solution

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13
Q

standard solution

A

a solution of a known concentration normally used in titrations to determine unknown info about another substance

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14
Q

conc (moldm-3) =

A

moles/volume

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15
Q

conc (gdm-3) =

A

mass/volume

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16
Q

no. moles of a gas=

A

volume/24

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17
Q

empirical formula

A

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

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18
Q

molecular formula

A

the actual numbet of atoms of each element in a molecule

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19
Q

molecule

A

small group of atoms held together by covalent bonds

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20
Q

what colour is methyl orange indicator in

a) acid
b) base
c) endpoint

A

a) red
b) yellow
c) orange

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21
Q

what colour is phenolphthalein indicator in

a) acid
b) base
c) endpoint

A

a) colourless
b) pink
c) pale pink

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22
Q

what is the colour of bromothymol blue indicator in

a) acid
b) base
c) endpoint

A

a) yellow
b) blue
c) green

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23
Q

acid

A

a species that is a proton donor

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24
base
species that is a proton acceptor
25
alkali
soluble base in water forming hydroxide ions
26
cation
positively charged ion
27
hydrated salt
crystalline compound containing water molecules
28
anion
negatively charged ion
29
anhydrous salt
substance that contains no water molecules - | the form without water
30
water of crystallisation
water molecules that form an essential part of the crystalline structure of a compound
31
species
any type of particle that takes place in a chemical reaction
32
oxidisation number
a measure of the number of electrons that an atom uses to bond with atoms of another element
33
oxidisation no for 'uncombinded element'
0
34
oxididation no for 'combined oxygen'
-2
35
oxidiation no for 'combined hydrogen'
+1
36
oxidation no for 'combined fluorine'
-1
37
oxyanions
negative ions that contain an element along with oxygen
38
oxidation
loss of electrons or an increase in oxidation numbet
39
reduction
gain of electrons or a decrease in oxidation number
40
redox reaction
reaction where both reduction and oxidation happen
41
first ionisation energy of an element
the energy required to remove 1 electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
42
electron sheilding
the repulsion between electrons in different inner shells. Sheilding reduces the net attractive force from the positive nucleus on outer-shell electrons
43
successive ionisation energy
a measure of the energy required to remove each electron in turn from 1 mole of gaseous atoms
44
shell
group of atomic orbitals with the same principal quantum number, n. Also known as main energy level
45
sub-shell
group of the same type of atomic orbitals (s,p,d and f) within a shell
46
orbital
region, or volume of space, within an atom that can hold up to 2 electrons with, opposite spins
47
electron configuration
arrangement of electrons in an atom
48
compound
a substance formed when 2 or more different elements chemically bond together in a fixed ratio
49
ionic bond
the electrostatic attraction between oppositely charged ions
50
covalent bond
bond formed by a shared pair of electrons
51
giant ionic lattice
3-D structure of oppositely charged ions bonded together by strong electrosatic forces
52
lone pair
the outer-shell pair of electrons that is not involved in chemical bonding
53
bond pairs
pairs of electrons that are shared between 2 atoms
54
dative covalent or coordinate bond
a shared pair electrons where both of the electrons have been provided by one of the bonding atoms only
55
trigonal planer
bond angle= 120 3bp 0lp
56
linear
bond angle = 180 2bp 0lp can have double bonds but ignore and pretend ' 2 bonding regions'
57
tetrahedral
bond angle = 109.5 4bp 0lp
58
octahedral
bond angle = 90 6bp 0lp
59
pyradimal
bond angle = 107 3bp 1lp
60
non-linear
104.5 bond angle 2bp 2lp
61
electronegativity
ability of an atom to attract the bonding electrons in a covalent bond - measure of attraction of a bonded atom for the pair of electrons in a covalent bond
62
permanent dipole
a small charge difference across a bond that results from a difference in the electronegativities of the bonded atoms
63
polar covalent bond
has a permanent dipole
64
how does a permanent dipole arise
when covalently-bonded atoms have different electronegativities, resulting in a polar bond
65
polar molecule
has an overall dipole, when you take into account any dipoles across the bonds
66
the greater the difference between the electronegativities of the bonding atoms....
the greater the ionic character of the bond
67
the greater the similarity in electronegativities of the bonding atoms....
the greater the covalent character of the bond
68
internolecular force
attractive force between neighboring molecules
69
permanent dipole-dipole force
a weak attractive force between PERMANENT DIPOLES in neighboring polar molecules
70
van der waals forces
attractive forces between INDUCED DIPOLES in neighbouring molecules
71
hydrogen bond
strong dipole-dipole attraction between: - an electron-deficient hydrogen atom (O or N) on one molecules - a lone pair of electrons on a highly electronegative atom (H-O or H-N) on a DIFFERENT MOLECULE
72
special properties of water
- ice is less dense than water (ice floats) | - water has relatively high melting and boiling points than expected for a small molecule
73
metallic bonding
electrostatic attraction between positive metal ions and negative delocalised electrons
74
delocalised electrons in metallic bonding
shared between more than 2 atoms
75
giant metallic lattice
a 3D structure of positive ions and delocalised electrons bonded together by strong metallic bonds
76
simple molecular lattice
3D structure of molecules, bonded together by weak IMF
77
giant covalent lattice
3D structure of atoms, bonded together by strong covalent bonds
78
period
horizontal row of elements in the Periodic Table - elements show trends in properties across a period
79
group
vertical column in Periodic Table. Elements in a group have similar chemical properties and their atoms have the same number of outer-shell electrons
80
periodicity
regular periodic variation of properties of elements with atomic number and position in Periodic Table. REPEATING PATTERN ACROSS DIFFERENT PERIODS
81
across a period what is the most important factor influencing ionisation energy
increased nuclear charge
82
down a group what is the most important factors influencing ionisation energy
increase distance and sheilding
83
thermal decomposition
breaking up of a chemical substance with heat into at least | two chemical substances
84
displacement reaction
a reaction in which a more-reactive element displaces a less-reactive element from an aqueous solution of the latter's ions
85
disproportionation
reaction in which an element is simultaneously oxidised and reduced as a redox reaction
86
precipitation reaction
formation of an insoluble solid from 2 solutions in a chemical reaction
87
atom
smallest particle of an element that retains its chemical properties

Chemistry Unit 1 AS (3 decks)

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