atomic and electronic structure

Question 1

name and describe the 7 people/models for the history of the atom

Answer 1

1. Democritus (5th century BC)
   atom was a tiny hard incurable shape
2. John Dalton (1803)
   Solid sphere. all matter is made of atoms
3. JJ Thomson (1889)
   Plum pudding model - sphere of positive charge with negatively charged particles scattered
4. Curie (1911)
   discover radioactivity
5. Rutherford scattering experiment
6. Neils Bohr (1913)
   Electrons orbit nucleus in shell, each orbit has a fixed energy
   7.Schrodinger (1926) and Dirac (1928)
   probability to find electrons within space surrounding nucleus. Up to date atomic model

Question 2

which 3 particles are in an atom and found where?

Answer 2

electron - shells orbiting
proton- nucleus
neutron- nucleus

Question 3

charge of each sub particle

Answer 3

proton- +1
electron- -1
neutron - 0

Question 4

relative mass of each sub particle

Answer 4

proton- 1
electron - 1/2000
neutron - 1

Question 5

6
C
12
which is atomic number and which is atomic mass and what do they show?

Answer 5

atomic number - 6 (proton and electron)
atomic mass- 12 (proton+ neutron)

Question 6

how to work out proton, electron and neutron of an isotope?

Answer 6

e.g 1
H
1
would have 1 proton, 1 electron, 0 neutron

Question 7

working out proton, neutrons electrons of an ion

Answer 7

if charge is positive, take electrons away
if charge is negative add electrons
e.g 12
Mg2+
24
has 12 protons, 12 neutrons and 10 electrons

Question 8

relative atomic mass equation

Answer 8

(isotopic mass x relative abundance) + (isotopic mass x relative abundance) / 100

Question 9

methods to work out % relative abundance

Answer 9

tug of war method - work out which more abundant
mathematical method- solve for x

Question 10

what does heisenbergs uncertainty principle state

Answer 10

electrons are found in energy levels called shells
made of sub shells
made of orbitals

Question 11

what’s a subshell

Answer 11

a group of the same type of atomic orbitals in a shell

Question 12

name the orbitals

Answer 12

s p d f

Question 13

in shell number 1:
sub shell present?
orbitals in subshell?
max number of electrons in each subshell?
man number of electrons in shell?

Answer 13

s
1 x s
2
2

Question 14

in shell number 2:
sub shell present?
orbitals in subshell?
max number of electrons in each subshell?
man number of electrons in shell?

Answer 14

s, p
1 x s, 3 x p
2,6
8

Question 15

in shell number 3:
sub shell present?
orbitals in subshell?
max number of electrons in each subshell?
man number of electrons in shell?

Answer 15

s, p, d
1 x s, 3 x p, 5 x d
2,6,10
18

Question 16

in shell number 4:
sub shell present?
orbitals in subshell?
max number of electrons in each subshell?
man number of electrons in shell?

Answer 16

s, p, d, f
1x s, 3 x p, 5 x d, 7 x f
2,6,10,14
32

Question 17

shape of s orbital

Answer 17

sphere

Question 18

shape of p orbital

Answer 18

dumbell ( infinity sign)

Question 19

how many electrons can fit in an orbital?

Answer 19

2

Question 20

how many electrons in s subshell

Answer 20

2

Question 21

how many electrons in p subshell

Answer 21

6 (3 orbitals, 2 e- in each)

Question 22

how many electrons in d subshell

Answer 22

10 ( 5 orbital per subshell, 2 e- in each)

Question 23

how many electrons in f subshell

Answer 23

14 (7 orbitals, 2e- in each)

Question 24

how do boxes get filled in orbitals?

Answer 24

fill individually with arrows then add a double

Question 25

the aufbau principle

Answer 25

electrons fill orbitals of lowest energy first

Question 26

electron filling order ( configuration)

Answer 26

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 4d10, 4f14

Question 27

what groups in periodic table are each block (spdf) and what’s it mean

Answer 27

s- group 1 and 2 p- group 3,4,5,6,7,8 d- transition metals f-ionthanoids when writing electron structure it will finish in that block

Question 28

electron configuration anomalies on the first row of d block why?

Answer 28

Cr - 3p6,4s1,3d5 Cu- 3p6,4s1,3d10 make atom more stable

Question 29

m/z values are for

Answer 29

a single charged positive ion