Atomic Structure Flashcards
(22 cards)
What is the Atomic Number
The number of protons in an atom
What is the Mass Number
The total number of protons and neutrons in an atom
What is the Relative Atomic Mass
The average weighted mean mass of an atom of an elements relative to 1/12 of the mass of an atom of Carbon-12
What is the Relative Isotopic Mass
The average weighted mean mass of an isotope of an elements relative to 1/12 of the mass of an atom of Carbon-12
What is an Isotope
Atoms which have the same atomic number but a different mass number
What is the Relative Formula Mass
The average weighted mean mass of a formula unit relative to 1/12 of the mass of an atom of Carbon-12
What is the Relative Molecular Mass
The average weighted mean mass of a molecule relative to 1/12 of the mass of an atom of Carbon-12
What does a Mass spectrometer do
Separates the isotopes of an elements according to their mass
What are the flame test results?
Li+ = crimson
Na+ = yellow/orange
K+ = lilac
Ca2+ = brick red
Ba2+ apple green
Cu2+ green-blue
Why are s/p/d block elements called as such
Their outer electrons are in s/p/d sub shells
What are Heisenbergs Uncertainty, Aufbau and Pauli’s Exclusion principle
You cannot measure the position and momentum of an electron at the same time, electrons enter the lowest available energy level and electrons in the same orbital have opposite spin
What are the shapes of each orbital and how many are in each sub shell
S - ball, 1
P - dumbbell, 3
D - various shapes, 5
What subshell is filled earlier than expected
4s orbital before 3d
What is First Ionisation Energy
The energy required to convert one mole of gaseous atoms into gaseous ions with a single positive charge
What is Second Ionisation Enegry
The energy required to convert one mole of gaseous ions with a single positive charge into gaseous ions with a double positive charge
What is Third Ionisation Energy
The energy required to convert one mole of gaseous ions with a double positive charge into gaseous ions with a triple positive charge
How does Nuclear Charge affect Ionisation Energy
Higher nuclear charge means stronger force of attraction between outer electron and nucleus, increasing ionisation energy
How does Shielding affect Ionisation Energy
Inner electrons shield outer electrons from nuclear charge, decreasing ionisation energu
How does atomic radius affect ionisation energy
An increased atomic radius means weaker force of attraction between outer electrons and nucleus, decreasing ionisation energy
How does stability of subshells affect ionisation energy
Have filled or filled subshells are more stable them partially filled, increasing ionisation energy
Why does 1st I.E increase across the period
Increasing nuclear charge, decreased atomic radius and no change in shielding increases ionisation energy
Why are there exceptions to the general rule of 1st I.E increasing across the period
The 1st I.E decreases because the element before it has a half/fully filled subshell, and thus is very stabel
