Electron configuration

Question 1

explain electrons charge

Answer 1

Electrons have a
- ve charge
Overall Electrically Neutral

Question 1

what makes up an atom

Answer 1

sub atomic particles

Question 2

what is the area an electrons inhabits called

Answer 2

Electrons do not just move freely in the extranuclear space but are confined
to a particular region
Each of these regions are named Shells or Principal Energy Levels

Question 3

formula for amount of electrons in each shell

Answer 3

Each shell fills to 2n*2 where
n is the number of the shell

Answer 4

Electrons have more energy the further away from the nucleus

Question 5

why is electronic structure important?

Answer 5

Electronic structure is important because in principal
it can predict the reactivity of atoms and molecules!

Question 6

subdivision of electronic shells

Answer 6

Shells are divided up into subshells labelled s, p, d and f

Question 7

how are subshells numbered

Answer 7

Each of the subshells can be numbered and with this numbering they are classified into a specific orbital

Answer 8

Orbital: Region of space that can hold 2 electrons

Question 9

How do we label Orbitals?

Answer 9

1. Large number is the Shell or Principal Energy Levels
2. The small letter refers to the shape

Question 10

what does the letter s mean?

Answer 10

The letter
s means a spherical orbital.

Question 11

what does the letter p mean?

Answer 11

The letter
p means a two–lobed orbital
-x, y, or z subscript on a p orbital label indicate
s
the coordinate axes the two lobes

Question 12

what does the letter d & f mean?

Answer 12

The d and f orbitals has 5 and 7 differently shaped orbitals respectively

Question 13

define a filled orbital

Answer 13

In general a filled orbital is where you will find an electron pair 90-95%
of the time

Question 14

Why does an H atom have so many orbitals and only 1 electron?

Answer 14

Hydrogen: Why does an H atom have so many orbitals and only 1 electron?

Question 15

what is an orbital

Answer 15

An orbital is a potential space for an electron, it can be empty
Atoms can have many potential (empty) orbitals

Answer 16

Previously conceived Bohr model (electrostatic, planetary model of the atom) proven by atomic emission spectra unfortunately, failed in the case of other heavier atoms

Question 17

why does bohr model fail

Answer 17

Reason: does not predict electron-electron repulsion, other nucleus-electron attractions, also states the
electron is not allowed to occupy any of the spaces in between the orbits.

Answer 18

Need one more property to determine how the electrons are arranged Spin – electron spins like a top

Question 19

define the pauli exclusion principle

Answer 19

Pauli Exclusion Principle – an atomic orbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins.

Answer 20

Electrons fill into equivalent energy orbitals before pairing up

Each orbital holds 2 electrons and with their spins paired

Answer 21

Electrons are “happy” when they are paired up in an orbital

Electrons counted like the previous two examples are in the ground state
conformation

Answer 22

1. Atoms have a series of energy levels called Principal Energy Levels, which are
   designated by whole numbers (
   n = 1, 2, 3, etc.)- Principle Quantum Number
   Summary: Electronic Structure of Atoms
2. The energy of the level increases as the value of n increases.
3. Each principal energy level contains one or more types of orbitals,
   called subshells
4. The number of subshells in a
   given Principal Energy Levels
   also equals n.
5. The
   n value is always used to label the orbitals of a given principal level and
   is followed by a letter that indicates the type (shape) of the orbital (
   1
   s, 3
   p, etc.)
6. An orbital can be empty or it can contain one or two electrons, but never
   more than two. If two electrons occupy the same orbital, they must have
   opposite spins.
7. The shape of an orbital does not indicate the details of electron movement.
   It indicates the probability distribution for an electron residing in that orbital

Answer 23

The orbital or, space where two electrons are found, belong to a specific shell
For example: An atom with 7 electrons fills : 2 electrons in the first shell and
5 electrons in the second shell.
In orbitals, electrons fill two into the 1s orbital, two into 2s orbital
and one into 2px, one into 2py and one into 2pz

Answer 24

Aufbau principle (German: build up) and order of orbital filling: In the ground state of an atom or even ions: electrons fill atomic orbitals, also obeying the Pauli Exclusion principle, in the lowest available energy levels before filling the higher levels. Order of Orbital and Subshell Filling 1. Each electron in an atom occupies the most stable available orbital 2. No two electrons can have identical quantum numbers 3. Orbital capacities are as follows: s: 2 electrons, p set: 6 electrons d set: 10 electrons, f set: 14 electrons.

Question 25

Core electrons definition

Answer 25

– Inner electrons

Question 26

Valence electrons definition

Answer 26

Electrons in the outermost (highest) principal energy level of an atom

Answer 27

The elements in the same group on the periodic table have the same valence electron configuration Elements with the same valence electron arrangement show very similar chemical behaviour