Atomic structure

Question 1

What are the subatomic particals and where are they?

Answer 1

proton–charge= + mass=1 found in nucleus
neutron– charge=neutral mass=1 found in nucleus
electron–charge=- mass=1/2000 orbit in shell around nucleus

Question 2

what are atoms made up of?

Answer 2

nucleus-a very dense and small,where the protons and neutrons are

shell-where the electrons orbit the atom

most of the atom is empty space

They are also neutral so have the same number of protons and electrons

Question 3

What does the number of protons tell us

Answer 3

The number of electeons and also what element it is

Question 4

what does the atomic number tell us?

Answer 4

it is equal to the number protons in the nucleus of an atom of that element, also tells which element it is

Question 5

what does the atomic mass number tell us?

Answer 5

it is equal to the mass number of protons+ the number of neutrons in the nucleus ( it tells us the mass of 1 atom of that element)

to calc no of neutrons do mass number- atomic number

Question 6

Isotope definition

Answer 6

isotopes are atoms of the same element ( same number of protons and electrons) with different number of neutrons

Question 7

differences and similarities between isotopic atoms of the same element

Answer 7

different masses
different numbers of neutrons
different physical properties (as this is decided by neutrons)

same number of protons and electrons
same chemical properties( as this is determined by electron)

Question 8

what is a cation

Answer 8

A positively charged ion

Question 9

what is a anion

Answer 9

A negatively charged ion

Question 10

how are ions formed

Answer 10

Atoms gain or lose electrons to form ions, by transferring or sharing them

if they gain electrons they become negative ion (non metals do this)

if they lose electrons they form positive ions (metals do this and Roman numerals are used to show positive charges sometimes)

Question 11

what is an ion

Answer 11

A charge partical

Question 12

Which subshells does each shell contain?

Answer 12

Sub shells
shell 1 = 1s sub-shell
shell 2 = 2s sub-shell + 2p sub-shell
shell 3 = 3s sub-shell + 3p sub-shell + 3d sub-shell
shell 4 = 4s sub-shell + 4p sub-shell + 4d sub-shell + 4f sub-shell

Question 13

what are subshells made up of

Answer 13

sub shells are made up of orbitals these are regions of space in an atom that can hold up to 2 electrons with opposite spins
there are 4 types S P D and F

Question 14

What are the s subshells made up of

Answer 14

They are made up of 1 s orbital
s orbitals are spherical in shape and can hold 2 electrons with opposite spins

Question 15

What are p sub shells made up of

Answer 15

3 P orbitals py pz and px
each P orbital has a dumbell shape
they each hold 2 electrons meaning a P sub shell can hold up too 6 electrons
electrons constantly move around the nucleus within this regin

Question 16

What are d sub shells made up of?

Answer 16

5 d orbitals
each of them can hold 2 electrons with opposite spins so all together a d sub shell can hold up too 10 electrons

Question 17

What are F sub shells made up of

Answer 17

7 F orbitals
each one can hold up to 2 electrons with opposite spins so a F sub shell can hold up too 14 electrons

Question 18

how many electrons can each shell hold

Answer 18

Shell 1- 1s sub shell can hold 2, so shell 1 can hold 2 electrons overall

Shell 2- 2s sub shellcan hold 2 and a 2p subshell which can hold 6, so shell 2 can hold up to 8 overall

Shell 3- 3s can hold 2 3p can hold 6 3d can hold 10, so 18 overall

shell 4- 4s can hold 2 4p can hold 6 4d can hold 10 4f can hold 14, so 32 overall

Question 19

how is the electron configuration of an atom shown ?

Answer 19

it is show by the subshells for example sodium ( atomic number of 11) is

1s² 2s² 2p⁶ 3s¹

This shows which subshells in each shell contain the electrons for example the S subshell in the 3rd shell and also how many they contain through the small
numbers for example 3s¹ means it contains 1 electron

Question 20

Relative isotopic Mass defintion

Answer 20

The relative isotopic Mass is the Mass of an atom of an isotope compared with 1/12th of the Mass of carbon-12

Question 21

Relative atomic mass definition

Answer 21

is the weighted mean mass of an atom of an element compared with 1/12th of an atom of carbon-12
Takes into account the percentage abundance of each isotope
and relative Mass of each isotope

Question 22

what is mass spectrometry used for?

Answer 22

To determine info about isotopes including their mass number and relative abundance

Question 23

Calc relative atomic mass

Answer 23

(atomic mass×percentage abundance)+( atomic mass × percentage abundance) / 100

Question 24

Atomic orbital definition

Answer 24

A region within an atom, around the nucleus, that can hold up to two electron, with opposite spins

Question 25

Shell defention+ properties

Answer 25

A group of atomic orbitals with the same principle quantum number
the shell closest to the nucleus has the lowest enrgy

Question 26

What are sub shells

Answer 26

They are a group of the same type of atomic orbitals within a shell

Question 27

Order of filling of the orbitals

Answer 27

Lowest energy fills first (closest to the nucleus)
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶…
4s² fills first as it has a lower energy than 3d¹⁰ it also loses electrons first when they become an ion

Question 28

Transition elements info

Answer 28

A transition element is a d-block element that forms and ion with an incomplete d sub- shell
they lose their 4s electrons first when forming positive ions
Cr and Cu also only fill 4s¹ before moving onto the 3d subshell as a exception to the 4s²