Atomic Structure And Periodicity

Question 1

Atom definition

Answer 1

smallest particle of an element.

Question 2

Element definition

Answer 2

composed of the same type of atom.

Question 3

Compound definition

Answer 3

two or more elements chemically bonded together.

Question 4

Molecule definition

Answer 4

two or more atoms covalently bonded together.

Question 5

Ion definition

Answer 5

Charged particle

Question 6

Cation definition

Answer 6

Positively charged ion

Question 7

Anion definition

Answer 7

Negatively charged ion

Question 8

Nucleon definition

Answer 8

Nucleons are the sub-atomic particles that exist in the nucleus of atoms (protons & neutrons).

Question 9

Strong nuclear force definition

Answer 9

The strong nuclear force holds together protons & neutrons in the nucleus

Question 10

Electrostatic forces of attraction definition

Answer 10

Electrostatic forces of attraction exist between any positive and negative particles.

Question 11

Isotopes definition

Answer 11

Isotopes are atoms of the same element with different numbers of neutrons. (same numbers of protons and electrons)

Question 12

Relative atomic mass definition

Answer 12

Relative atomic mass (Ar) is the average mass of an atom of an element (taking into account the relative abundances of isotopes) compared to one twelfth of the mass of one atom of carbon-12

Question 13

Relative isotopic mass

Answer 13

Relative isotopic mass is the mass of an atom of an isotope compared to one twelfth of the mass of one atom of carbon-12.

Question 14

Atomic number definition

Answer 14

Atomic number (Z) is the number of protons in the nucleus of an atom of that element

Question 15

What does ‘A’ mean?

Answer 15

A = mass number (no. of protons + neutrons in the nucleus)

Question 16

Species definition

Answer 16

A species in chemistry is “a substance composed of chemically identical entities”

Question 17

Relative molecular mass definition

Answer 17

Relative molecular mass (Mr) of a compound is the sum of the relative atomic masses of all the atoms in a molecule compared to one twelfth of the mass of one atom of carbon-12.

Question 18

Relative formula mass definition

Answer 18

Relative formula mass (Mr) of an ionic compound is the sum of the relative atomic masses of all the atoms in the formula compared to one twelfth of the mass of one atom of carbon-12.

Question 19

Main shell/ quantum shell definition

Answer 19

A main shell or quantum shell is made up of sub-shells containing orbitals, where electrons are found.

Question 20

Orbital definition

Answer 20

An orbital is a region of space in an atom containing up to two electrons with opposite spins.

Question 21

Sub shell definition

Answer 21

A sub-shell is one or more orbitals in the same shell which have the same energy levels.

Question 22

Block element definition

Answer 22

A _-block element has its highest energy electron in an _ orbital (replace _ with s/p/d/f), i.e…

Question 23

S block element definition

Answer 23

An s-block element has its highest energy electron in an s orbital

Question 24

P-block element definition

Answer 24

A p-block element has its highest energy electron in a p orbital

Question 25

D block element definition

Answer 25

A d-block element has its highest energy electron in a d orbital

Question 26

Transition metals definition

Answer 26

Transition metals are elements which form at least one stable ion with partially filled d orbitals.

Question 27

First ionisation energy definition

Answer 27

First ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state. [ M(g) → M+(g) + e- ]

Question 28

Second ionisation energy definition

Answer 28

Second ionisation energy is the energy required to remove one mole of electrons from one mole of 1+ ions in the gaseous state. [ M+(g) → M2+(g) + e- ]

Question 29

Successive ionisation energy definition

Answer 29

Successive ionisation energy is the energy required to remove the electrons one after the other.

Question 30

Periodicity definition

Answer 30

Periodicity is a regularly repeating pattern of atomic, physical and chemical properties with increasing atomic number.

Question 31

What are the 5 parts of the mass spectrometer?

Answer 31

~ A sample inlet- ~ An ionisation chamber- ~ X (g) + e- → X+ (g) + 2e- An electric field to accelerate- ~ A magnetic field to deflect- ~ Those with greater mass are deflected less than those with smaller mass. ~ The angle of deflection depends on the ______________

Question 32

What are the uses of the mass spectrometry?

Answer 32

- To determine isotopic composition - To determine the relative molecular mass of a molecule - To determine relative atomic mass of an element e.g - To determine drugs in urine samples-e.g anabolic steroid nandrolene have a unique molar mass - In the pharmaceutical industry- - Carbon-14 dating-

Question 33

What is the definition of fragmentation?

Answer 33

i.e breakdown of X+ into lighter positively charged ions

Question 34

Nuclear charge definition

Answer 34

The charge of the nucleus

Question 35

Electron shielding definition

Answer 35

Outer shell electrons don’t experience the force of attraction of nucleus due to the presence of inner shell electrons

Question 36

What’s the 1st quanta?

Answer 36

Has only 1 orbital, it’s an S and is a sphere. Can take up to 2 electrons with opposite spins

Question 37

What is the 2nd quanta?

Answer 37

Has 3 orbitals with letter P, dumbell shape can take up to 6 electrons

Question 38

What other blocks are there other than s and p?

Answer 38

D block- up to 10 electrons and 5 orbitals F block- up to 14 electrons and 7 orbitals

Question 39

Order of electron configuration

Answer 39

1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 6s 6p 7s Goes diagonally from right to left (downwards)

Question 40

Exceptions for the order of electron configuration

Answer 40

Cr is 3d^5 4s^1 NOT 3d^4 4s^2 Cu is 3d^10 4s^1 NOT 3d^9 4s^2

Question 41

What is ionisation energy affected by?

Answer 41

~ size ~ nuclear charge ~ shielding

Question 42

What happens to the ionisation energy as you move down a group?

Answer 42

- ionisation energy decreases - because size increases, as there are more shells, so forces of attraction increase - the nuclear charge increases as there’s more protons - the shielding increases as the shell number increases, less attraction between outer shell electrons and nucleus due to inner shell electrons

Question 43

What happens to the ionisation energy as you move along a period?

Answer 43

- as you go along the period, the ionisation energy increases - because the size decreases due to electrons being removed from the same shell - the nuclear charge increases as there are more protons, and more forces of attraction between the electrons and the protons - shielding does not change as no new shells are added

Question 44

Electronegativity definition

Answer 44

Extent that an element can attract a bonding electron to itself, fluorine is the most electronegative element