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Hint
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Answer
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Atoms of same element with different mass numbers
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Isotopes
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Technique used to find molecular mass of elements and compounds
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Mass spectrometry
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On a mass spectra, from what you can calculate the relative abundance of each ion in a sample? (Height of each ____)
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Peak
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What is the mass to charge (m/z) ratio equal to? (____ of detected ion)
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Mass
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Reaction where two light atomic nuclei fuse to form a heavier one
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Nuclear fusion
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Kind of radiation that a substance can emit or absorb
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Electromagnetic
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Star’s surface
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Photosphere
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Layer outside star’s surface that contains ions, atoms and small molecules
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Chromosphere
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These absorb some of radiation emitted, so light analysed from stars is missing some frequencies, creating an ____ ____
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Absorption spectrum
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When the particles absorb energy, raised from ___ ___ to an excited state
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Ground state
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Can lose energy by emitting EM radiation, creating an ____ ____
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Emission spectrum
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These disrupt a spectrum that is ordinarily ____
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Continuous
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Hydrogen emission spectrum in UV light
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Lyman series
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Theory that describes behaviour of light
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Wave-particle duality
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3.0x10^8
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Speed of light/c
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Speed of light = wavelength ____ by frequency
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Multiplied
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What varies the colour of visible light
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Wavelength
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Particle theory: light regarded as stream of energy packets called ____
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Photons
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Energy of photon (J) = Plank constant (Js^-1) ____ by frequency (s^-1)
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Multiplied
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6.63x10^-34
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Planck constant/h
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Man who came up with theory to explain why hydrogen atom only emits specific frequencies
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Bohr/Niels Bohr
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Theory relied on theory of ____ of energy
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Quantisation
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Main point 1: ____ in hydrogen atom only exists in certain definite electron shells
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Electron
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2: A ____ is emitted or absorbed when the electron changes from one level to another
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Photon
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3: Energy of photon equal to ____ between energy levels
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Difference
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4: Frequency of emitted/absorbed light: energy change = __ x __.
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hv
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Electron can only possess definite quantities of energy: ____
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Quanta
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The larger the energy gap between the two levels, the ____ the frequency of EM radiation emitted
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Higher
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Maximum number of electrons shell 1 can hold
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2
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Maximum number of electrons shell 2 can hold
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8
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Maximum number of electrons shell 3 can hold
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18
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Maximum number of electrons shell 4 can hold
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32
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What are the sub-shells labelled (in order)?
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spdf
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Maximum number of electrons sub-shell s can hold
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2
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Maximum number of electrons sub-shell p can hold
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6
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Maximum number of electrons sub-shell d can hold
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10
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Maximum number of electrons sub-shell f can hold
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14
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Number of orbitals in the sub-shell = maximum number of electrons divided by ____
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2
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In an ____ atom, orbitals in same sub shell have same energy
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Isolated
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Position of electron can’t be mapped exactly – we can only know the ____ of finding the electron in a given atomic orbital
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Probability
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Electrons have a ___ and two can only occupy the same orbital if they have paired ones
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Spin
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Shape of s orbital
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Sphere/spherical
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Shape of p orbital
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Dumbbell/peanut
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Arrangement of electrons in shells
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Configuration
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Orbitals filled in order of ____ energy
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Increasing
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The occurrence of periodic patterns (properties vary in a fairly regular way as you go left to right)
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Periodicity
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Group 1 and 2: ____ block
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s
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Transition metals: ____ block
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d
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Groups 3-8: ____ block
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p
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Lanthanides and actinides: ____ block
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f
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Pattern in ____ and ____ points across a period: initially increase, then fall dramatically, then decrease slowly
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Melting boiling/boiling melting
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Electronic configuration where sub-shells are fully occupied by electrons: ____-____ arrangement
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Closed shell
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Shared pair of electrons
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Covalent bond
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Pairs of electrons not involved in bonding
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Lone pairs
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Covalent bond where both electrons in a pair come from the same atom
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Dative
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Shown by an arrow pointing away from the atom that ____ the pair
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Donates
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Bond angle of tetrahedral molecules
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109.5
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