atomic structure and electron configuration

Question 1

atomic number =

Answer 1

number of protons

Question 2

number of protons=

Answer 2

number of electrons(in neutral atom)

Question 3

Isotopes

Answer 3

atoms of the same element which contain different number of neutrons

Question 4

of neutrons =

Answer 4

mass number - atomic number

Question 5

in isotope notation state where the mass # is and the atomic number

Answer 5

mass number on the top

atomic number below mass number

Question 6

how are ions formed

Answer 6

when atoms gain or lose electrons when reacting chemically

Question 7

in ionically charge atoms does # of protons equal # of electrons

Answer 7

no

Question 8

how to find relative atomic mass?

Answer 8

divided percentages by 100 then multiply that number by the mass number that goes along with that percentage. there should be addition between each parenthesis

Question 9

energy level shell: max # of electrons

Answer 9

1:2
2:8
3:18
4:32

energy level on left, max # of electrons on right

Question 10

sub level: max # of electrons

Answer 10

S:2
P:6
D:10
F:14

Question 11

which level gets removed before: level 4 electrons or 3d

Answer 11

level 4, because level is lower in energy due to less electron repulsion

Question 12

electron configuration example

Answer 12

1s2,2s2,3p6 and so on

Question 13

Chronium electron configuration(24e)

Answer 13

1s2,2s2,2p6,3s2,3p6,4s1,3d5

instead of having 4s2 ad 3d4 write 4s1 3d5

same goes with copper: write 4s1 3d9

Question 14

Orbitals

Answer 14

think of them as the boxes

can only contain a max of two electrons in each box

Question 15

sub level: # of orbitals

Answer 15

S:1
P:3
D:5
F:7

Question 16

drawing of orbitals( explain what the 4 different variations are

Answer 16

S= spherical

Px= dumbbell across x axis

Py= dumbbell across y axis

Pz= diagonal dumbell

Question 17

electron configuration of ions

Answer 17

if the charge is + then remove

if the charge is negative then add