Topic 3.1.1 Atomic Structure

Question 1

Atoms

Answer 1

The smallest particles into which an element can be divided and still remain their characteristic properties

Question 2

Proton

Answer 2

A positively charged subatomic particle found in the nucleus

Question 3

Neutron

Answer 3

A subatomic particle Found in the nucleus which has zero charge and very nearly the same mass as the proton

Question 4

Electron

Answer 4

A negatively charged subatomic particle about 1/1836 of the mass of a proton. In neutral atoms, the number of electrons equal number of protons. It is only the outer (valentine shell) Electrons which take part in bonding and in chemical reactions

Question 5

Atomic number Z

Answer 5

The number of protons in the nucleus of an atom the same as atomic number

Question 6

Mass number A

Answer 6

The number of protons and the number of neutrons

Question 7

Isotopes

Answer 7

Atoms which contain the same number of protons but different number of neutrons. Nearly all the elements Consist of mixtures of isotopes, formed inside stars in the early stages of the universe. Isotopes of the same element have the same chemical properties as they all have the same electron configuration

Question 8

Relative isotopic mass

Answer 8

Relative isotopic mass is a mass of an atom of an isotope of an element relative to 1/12 the atomic mass of an atom of carbon 12

Question 9

Relative atomic mass AR

Answer 9

Ar = average mass of an atom/ 1 12th mass of 1 atom of c12

Question 10

Ionisation energy

Answer 10

The energy required to remove a mole of electrons from one mole of isolated gassiest atoms or ions.

Question 11

First ionisation energy

Answer 11

The entropy change when one mole of electrons is removed from one mole of gaseous atoms, forming one mole of gaseous singly charge cations

X(g) —> X+(g) + e-

Question 12

Second ionisation energy

Answer 12

And to be change when one mole of electrons is removed from one mole of singly charge gaseous cat ions from one mole of doubly charge gaseous cations

X+(g)—> x*2+ (g) + e-

Question 13

Nth ionisation energy

Answer 13

The enthalpy change when one mole of electrons is removed from one mole of (N-1) charge gaseous cations forming one mole of N- charge gaseous cations

X^(n-1)+gas —> x^N+(g) +e-

Question 14

Successive ionisation energies

Answer 14

The ionisation energy values for removing the second and subsequent electrons

Question 15

Atomic radius

Answer 15

A measure of the size of an atom.

Question 16

First electron affinity

Answer 16

The enthalpy change when one mole Of electrons is added to one mole of gaseous singly charge and I want to produce one mole of gaseous doubly charged anions

X(g) + e- —> x- (g)

Question 17

Second electron affinity

Answer 17

The enthalpy change when one mole of electrons are added to one mole of gassiest singly charged anions to produce one mole of gassiest doubly charged anions

Question 18

Electron configuration

Answer 18

The arrangement of electrons in an atom or ions

Question 19

Ground state

Answer 19

The lowest energy state of an atom

Question 20

Excited state

Answer 20

An energy state of an atom which is higher than the ground state

Question 21

Electron shell

Answer 21

Main energy levels described by a number

Question 22

Build up principal

Answer 22

Lower energy orbitals are feeling before higher energy orbitals.

half full subshells and full subshells a particularly stable

Question 23

Orbital

Answer 23

The volume of space in which there is a 95% probability of finding an electron

Question 24

S-Block element

Answer 24

Certain atoms which the last electron added enters an S orbital e.g. sodium

Question 25

P – block elements

Answer 25

Certain atoms in which the last electron added enters a P orbital e.g. aluminium

Question 26

D - block elements

Answer 26

Certain atoms in which the last electron added enters a D orbital e.g. scandium