1. Atomic Structure Flashcards
Describe an atom
atoms are mostly empty space surrounding a very small, dense nucleus that contains protons and neutrons; electrons are found in shells in the empty space around the nucleus
describe subatomic particles- protons, neutrons and electrons in terms of their relative charges and relative masses
mass- 1, 1, 1/1836
charge- +1, 0, -1
Explain the terms atomic and proton number; mass and nucleon number
describe the distribution of mass and charge within an atom
describe the behavior of beams of protons, neutrons and electrons moving at the same velocity in an electric field
neutrons are uncharged so go straight.
proton deflect towards -ve
electron deflects towards +ve
electros deflect more as higher charge to mass ratio so acceleration increases.
determine the numbers of protons, neutrons and electrons present in both atoms and ions given atomic or proton number, mass or nucleon number and charge
state and explain qualitatively the variations in atomic radius and ionic radius across a period and down a group
define the term isotope and its notation
isotopes are atoms of the same element with same number of protons and different number of neutrons.
x^Ay
for isotopes, where x is the mass or nucleon number and y is the atomic or proton number
state that and explain why isotopes of the same element have the same chemical properties
state that and explain why isotopes of the same element have different physical properties, limited to mass and density
understand the terms:
* shells, sub-shells and orbitals
* principal quantum number (n)
* ground state, limited to electronic configuration
shell-
subshell-
orbitals-
principal quantum number-
ground state-
describe the number of orbitals making up s, p and d sub-shells, and the number of electrons that can fill s, p and d sub-shells
s- 1 orbital 2e-
p- 3 orbitals 6e
d- 5 orbitals 10e
f- 7 orbitals 14e
describe the order of increasing energy of the sub-shells within the first three shells and the 4s and 4p
sub-shells
determine the electronic configuration of atoms and ions given the atomic or proton number and charge,
using either of the following conventions:
understand and use the electrons in boxes notation
Fe: 1s2 2s2 2p6 3s2 3p6 3d6 4s2 (full electronic conf)
[Ar] 3d64s2 (shorthand electronic configuration)
describe and sketch the shapes of s and p orbitals
describe a free radical
s orbital-
p- orbital x,y,z axis
species with one or more unpaired electrons
define and use the term first ionisation energy, IE
construct equations to represent first, second and subsequent ionisation energies
explain the trends in ionisation energies across a period and down a group
explain the variation in successive ionisation energies of an element
explain the factors influencing the ionisation energies of elements and what causes them
nuclear charge- ii
atomic/ionic radius- id
shielding by inner shells and sub-shells- id
spin-pair repulsion-
all due to the attraction between the nucleus and the outer electron.
exceptions of configuration
bw 2nd & 3rd-
bw 5th & 6th-
