Atomic Orbitaks, Electronic Configuration And Perioc Table

Question 1

How to electrons behave in an atom

Answer 1

Behave as standing waves in an atom. These are aves that vibrate in time but do not move in space

Question 2

Describe orbitals

Answer 2

Different sizes and shapes of standing wave possible around the nucleus. Orbitals an hold a maximum of two electrons

Question 3

How many orbitals are ther

Answer 3

4-s,p,d and f

Question 4

What are atomic orbitals

Answer 4

Regions where there is a high probability of finding the electrons

Question 5

What are the 4 quantum numbers

Answer 5

Principle quantum number (n). Angular momentum quantum number (Ms). Magnetic quantum number (Ml). Spin magnetic quantum number (Ms)

Question 6

What does an orbital hold

Answer 6

A maximum of two electrons with opposite spin

Question 7

What are the orbitals in an isolated atom

Answer 7

Each shell is said to be degenerate

Question 8

What are atomic orbitals

Answer 8

The regions where there is a high probability of finding an electron

Question 9

Describe s orbitals

Answer 9

All s orbitals a spherical in shape. Their diameter increases as the shell number increases. The only orbital present in the first shell

Question 10

Describe p orbitals

Answer 10

Dumbbell shape. Only occur from the second shell onwards. These orbitals have equal energy and are said to be degenerate. Second shell has 1s and 3p orbitals

Question 11

Describe the 3rd shell

Answer 11

Can hold a maximum of 18 electrons. Two electrons are held in the s orbital and another six are held in the three p orbitals meaning 10 electrons are held in the d orbitals therefore 5 d orbitals in the third shell

Question 12

What shows evidence of atomic orbitals

Answer 12

Emission spectra of elements with more tHan on electron

Question 13

What’s quanta

Answer 13

Certain fixed amounts of energy posed by an electron

Question 14

Whats the quantum theory

Answer 14

States that the energy if an electron can be defined in terms of for quantum numbers

Question 15

Whats principles quantum number

Answer 15

Each shell is described by a number known as this. This number indicates the electrons main energy level and related to orbital size. First shell n=1 and so on

Question 16

The higher the value fo the principle quantum number the what

Answer 16

The higher the potential energy associated with the shell and the further from the nucleus the electron is likely to be found

Question 17

What’s angular momentum quantum number

Answer 17

The shape of the sub shell is given by this. If value l=0 the electron is found in the s orbital, if l=1 electron found in the p orbital and so on

Question 18

Whats magnetic quantum number

Answer 18

The orientation in space of the electron in different degenerate orbitals values between -1 and +1

Question 19

Whats spin magnetic quantum number

Answer 19

Indicates the direction in which the electron is spinning its either clockwise or anticlockwise with values +1/2 and -1/2 electrons occupying the same orbital must have opposite spins

Question 20

What are the orbitals within each subshell of an isolated atom

Answer 20

They are degenerate

Question 21

What does the Pauli exclusion state

Answer 21

That no two electrons in one atom can have the same set of four quantum numbers. In other words no orbital can hold more than two electrons and they must have oppsite spins

Question 22

Whats the aufbau principle

Answer 22

States that orbitals are filled in order of increasing energy

Question 23

What is hunds rule

Answer 23

States that when degenerate orbitals are available/ electrons fill singly keeping their spins parallel before spin pairing starts

Question 24

Whats the filling order for sub shells

Answer 24

1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s etc

Question 25

What is isoelectronic

Answer 25

Particles which have the same electronic configuration

Question 26

Learn copper and chromium electro ionic configuration of by heart as they don’t follow the rule

Question 27

Whats ground state

Answer 27

When electrons are in their lowest possible energy levels the atom is said to be in the ground state

Question 28

Learn how to right electronic configuration

Question 29

Learn how to write orbital box notation

Question 30

What provides evidence for the electronic configurations of sub shells

Answer 30

First, second and subsequent ionisation energies with increasing atomic number for the first 36 elements can be explained in terms of the relative stability of different subshell electronic configurations

Question 31

The more stable the electronic configuration

Answer 31

The higher the ionisation energy

Question 32

Whats the ionisation energy

Answer 32

The energy involved in removing one mole of gaseous atoms from one mole of atoms in the gaseous state

Question 33

What generally happens to ionisation energy across a period

Answer 33

Increases as electrons are being removed from the same shell and the nucleur charge increases along the period and so the outer electrons experience greater attraction.

Question 34

Why isn’t there a constant increases in ionisation energy across a period from group 2 to 3

Answer 34

The added electron is in the new p subshell which has a slightly higher energy level and is slightly further from the nucleus. The s2 electrons also provide shielding of group 3 elements

Question 35

Why isn’t there a constant increase in ionisation energy from group 5 to 6 and period 3

Answer 35

Due to the stability of the p orbitals

Question 36

The more stable the electronic configuration present the what

Answer 36

The harder it is to remove the outer electron from its attraction to the nucleus and the higher the ionisation energy

Question 37

What bits of the periodic table have what blocks

Answer 37

Hydrogen, helium and first two columns have s blocks Transition metals have d blocks Bottoms bit has f blocks Right side is p blocks

Question 38

What is a dative covalent bond

Answer 38

One in which one atom of the bond provides both electrons of the bonding pair

Question 39

What are lone pairs

Answer 39

Non bonding electron pairs

Question 40

Describe pairs of electrons

Answer 40

They are negatively charged and so repel each other. Arranged in a way so they are as far apart as possible so repulsion is minimised

Question 41

What is VSEPR theory used for

Answer 41

To predict the shapes of molecules and poly atomic ions

Question 42

What is the arrangement of electron pairs

Answer 42

Linear, trigonal, tetrahedral, trigonal bipyramidal, and octahedral

Question 43

Whats the order of decrease in electron pair repulsion’s

Answer 43

Lone pair-lone pair, lone pair-bonding pair, bonding pair-bonding pair

Question 44

When is a covalent bond formed

Answer 44

When two atomic orbitals combine together to form a molecular orbital

Question 45

What’s the number of electron pairs formula

Answer 45

Number of electron pairs= (electrons of central atom+ number of atoms attached) /2

Question 46

What name is given to each total number of electron pairs

Answer 46

2=linear 3=trigonal 4= tetrahedral 5= trigonometry bipyramidal 6= octahedral

Question 47

Whats the number of electron pairs for BrF4 -

Answer 47

7 central atoms + 1 charge electron (for the negative and - if it was positive) + 4 atoms attached divided by 2

Question 48

Describe lone pairs

Answer 48

Held closer to the central atom so they have greater repulsion than the bonding pairs of electrons

Question 49

Learn bi=one angles for tetrahedral, pyramidal and angular shapes

Question 50

What do lone pairs do to bond angles in tetrahedral

Answer 50

Cause it to decrease by 2.5 degrees for each lone pair

Question 51

Describe electrons

Answer 51

Behave as standing waves in an atom. These are waves that vibrate in time but do not move in space

Question 52

Whats can be explained by considering the electronic configurations

Answer 52

Anomalies in the trends of ionisation energies can be explained by considering the electronic configuration