|
Hint
|
|
Answer
|
|
Atoms of same element with different mass numbers
|
|
Isotopes
|
|
Technique used to find molecular mass of elements and compounds
|
|
Mass spectrometry
|
|
On a mass spectra, from what you can calculate the relative abundance of each ion in a sample? (Height of each ____)
|
|
Peak
|
|
What is the mass to charge (m/z) ratio equal to? (____ of detected ion)
|
|
Mass
|
|
Reaction where two light atomic nuclei fuse to form a heavier one
|
|
Nuclear fusion
|
|
Kind of radiation that a substance can emit or absorb
|
|
Electromagnetic
|
|
Star’s surface
|
|
Photosphere
|
|
Layer outside star’s surface that contains ions, atoms and small molecules
|
|
Chromosphere
|
|
These absorb some of radiation emitted, so light analysed from stars is missing some frequencies, creating an ____ ____
|
|
Absorption spectrum
|
|
When the particles absorb energy, raised from ___ ___ to an excited state
|
|
Ground state
|
|
Can lose energy by emitting EM radiation, creating an ____ ____
|
|
Emission spectrum
|
|
These disrupt a spectrum that is ordinarily ____
|
|
Continuous
|
|
Hydrogen emission spectrum in UV light
|
|
Lyman series
|
|
Theory that describes behaviour of light
|
|
Wave-particle duality
|
|
3.0x10^8
|
|
Speed of light/c
|
|
Speed of light = wavelength ____ by frequency
|
|
Multiplied
|
|
What varies the colour of visible light
|
|
Wavelength
|
|
Particle theory: light regarded as stream of energy packets called ____
|
|
Photons
|
|
Energy of photon (J) = Plank constant (Js^-1) ____ by frequency (s^-1)
|
|
Multiplied
|
|
6.63x10^-34
|
|
Planck constant/h
|
|
Man who came up with theory to explain why hydrogen atom only emits specific frequencies
|
|
Bohr/Niels Bohr
|
|
Theory relied on theory of ____ of energy
|
|
Quantisation
|
|
Main point 1: ____ in hydrogen atom only exists in certain definite electron shells
|
|
Electron
|
|
2: A ____ is emitted or absorbed when the electron changes from one level to another
|
|
Photon
|
|
3: Energy of photon equal to ____ between energy levels
|
|
Difference
|
|
4: Frequency of emitted/absorbed light: energy change = __ x __.
|
|
hv
|
|
Electron can only possess definite quantities of energy: ____
|
|
Quanta
|
|
The larger the energy gap between the two levels, the ____ the frequency of EM radiation emitted
|
|
Higher
|
|
Maximum number of electrons shell 1 can hold
|
|
2
|
|
Maximum number of electrons shell 2 can hold
|
|
8
|
|
Maximum number of electrons shell 3 can hold
|
|
18
|
|
Maximum number of electrons shell 4 can hold
|
|
32
|
|
What are the sub-shells labelled (in order)?
|
|
spdf
|
|
Maximum number of electrons sub-shell s can hold
|
|
2
|
|
Maximum number of electrons sub-shell p can hold
|
|
6
|
|
Maximum number of electrons sub-shell d can hold
|
|
10
|
|
Maximum number of electrons sub-shell f can hold
|
|
14
|
|
Number of orbitals in the sub-shell = maximum number of electrons divided by ____
|
|
2
|
|
In an ____ atom, orbitals in same sub shell have same energy
|
|
Isolated
|
|
Position of electron can’t be mapped exactly – we can only know the ____ of finding the electron in a given atomic orbital
|
|
Probability
|
|
Electrons have a ___ and two can only occupy the same orbital if they have paired ones
|
|
Spin
|
|
Shape of s orbital
|
|
Sphere/spherical
|
|
Shape of p orbital
|
|
Dumbbell/peanut
|
|
Arrangement of electrons in shells
|
|
Configuration
|
|
Orbitals filled in order of ____ energy
|
|
Increasing
|
|
The occurrence of periodic patterns (properties vary in a fairly regular way as you go left to right)
|
|
Periodicity
|
|
Group 1 and 2: ____ block
|
|
s
|
|
Transition metals: ____ block
|
|
d
|
|
Groups 3-8: ____ block
|
|
p
|
|
Lanthanides and actinides: ____ block
|
|
f
|
|
Pattern in ____ and ____ points across a period: initially increase, then fall dramatically, then decrease slowly
|
|
Melting boiling/boiling melting
|
|
Electronic configuration where sub-shells are fully occupied by electrons: ____-____ arrangement
|
|
Closed shell
|
|
Shared pair of electrons
|
|
Covalent bond
|
|
Pairs of electrons not involved in bonding
|
|
Lone pairs
|
|
Covalent bond where both electrons in a pair come from the same atom
|
|
Dative
|
|
Shown by an arrow pointing away from the atom that ____ the pair
|
|
Donates
|
|
Bond angle of tetrahedral molecules
|
|
109.5
|
|
How many lone pairs in tetrahedral molecules
|
|
0
|
|
How many bonded pairs
|
|
4
|
|
Bond angle of trigonal pyramidal molecules
|
|
107
|
|
How many lone pairs
|
|
1
|
|
How many bonded pairs
|
|
3
|
|
Bond angle of bent molecules
|
|
104.5
|
|
How many lone pairs
|
|
2
|
|
How many bonded pairs
|
|
2
|
|
Bond angle of linear molecules
|
|
180
|
|
How many groups of electrons around central atom
|
|
2
|
|
Bond angle of planar triangular molecules
|
|
120
|
|
How many groups of electrons around central atom
|
|
3
|
|
Bond angles of trigonal bipyramidal molecules
|
|
120 90/90 120
|
|
How many groups of electrons around central atom
|
|
5
|
|
Bond angle of octahedral molecules
|
|
90
|
|
How many groups of electrons around central atom
|
|
6
|
|
Mass of an atom of an element relative to carbon-12 (assigned mass of exactly 12)
|
|
Relative atomic mass/Ar
|
|
One ____ of substance contains as many particles are there are atoms in 12g of carbon-12
|
|
Mole/mol
|
|
____ ____ is equal to Ar of substance in grams
|
|
Molar mass
|
|
Substances are made up of ____ ____. Basic building blocks. Match formula of substance.
|
|
Formula units
|
|
Tells you the actual numbers of different types of atom
|
|
Molecular formula
|
|
Simplest ratio for moles of atoms in the formula
|
|
Empirical formula
|
|
Crystals of some ionic lattices include molecules of ____
|
|
Water
|
|
Fitted within lattice in regular manner. Called ____ ____ ____
|
|
Water of crystallisation
|
|
Crystals said to be ____
|
|
Hydrated
|
|
When heated, water removed as steam, leaving ____ solid
|
|
Anhydrous
|
|
When water added to anhydrous copper sulfate (____ colour) hydrated copper sulfate is formed (____colour)
|
|
White blue
|
|
To calculate formula: heat until ____ stops decreasing (all water evaporated)
|
|
Mass
|
|
Expected amount of product in a reaction under ideal conditions
|
|
Theoretical yield
|
|
Actual amount of product produced
|
|
Experimental yield
|
|
H2SO4
|
|
Sulfuric acid
|
|
HCl
|
|
Hydrochloric acid
|
|
HNO3
|
|
Nitric acid
|
|
CH3COOH
|
|
Ethanoic acid
|
|
Form when atoms lose electrons to form positively charged ions
|
|
Cation
|
|
Form when atoms gain electrons to form negatively charged ions
|
|
Anion
|
|
Metal + non metal forms an ____ bond
|
|
Ionic
|
|
Ions held together by opposite charges in ____ bond
|
|
Electrostatic
|
|
Acid + alkali -> ____ + ____
|
|
Salt + water
|
|
Acid + base -> ____ + ____
|
|
Salt + water
|
|
Acid + carbonate -> ____ + ____ + ____
|
|
Salt + water + carbon dioxide
|
|
Acid + metal -> ____ + ____
|
|
Salt + hydrogen
|
|
Acid + metal oxide -> ____ + ____
|
|
Salt + water
|
|
Compounds insoluble in water: barium, calcium, lead and silver ____
|
|
Sulfates
|
|
Silver and lead ____
|
|
Halides
|
|
All ____ ____ (except group 1 carbonates excluding lithium)
|
|
Metal carbonates
|
|
Metal hydroxides (except group 1 hydroxides and ____ ____)
|
|
Ammonium hydroxide
|
|
Ions not involved in reaction
|
|
Spectator
|
|
Suspension of solid particles produced by a chemical reaction in solution
|
|
Precipitate
|
|
Testing for ions - precipitate colour: copper + sodium hydroxide
|
|
Blue
|
|
Iron (II) + sodium hydroxide
|
|
Dirty green
|
|
Iron (III) + sodium hydroxide
|
|
Orange brown
|
|
Lead + potassium iodide
|
|
Bright yellow
|
|
Chloride + silver nitrate
|
|
White
|
|
Bromide + silver nitrate
|
|
Cream
|
|
Iodide + silver nitrate
|
|
Pale yellow
|
|
Sulfate + barium chloride
|
|
White
|
