atomic structure and periodic table

Question 1

the model of an atom consists of what?

Answer 1

a small nucleus and electrons in orbital

Question 2

who found this current model ?

Answer 2

rutherford

Question 3

how did rutherford find it

Answer 3

scattering experiment 1911

Question 4

what does the nucleus consist of?

Answer 4

protons and neutrons

Question 5

whats the charge of a nucleus

Answer 5

positive

Question 6

what is the atomic mass

Answer 6

the number of protons and neutrons

Question 7

how is the atomic mass represented

Answer 7

A

Question 8

what is the atomic number

Answer 8

the number of protons

Question 9

how is the atomic mass represented

Answer 9

z

Question 10

what is an isotope

Answer 10

different atom of the same element, same atomic number but different Atomic mass

Question 11

what is relative atomic mass

Answer 11

mass of an atom of an element relative to 1/12 t of the mean mass of C-12

Question 12

what is relative isotopic mass

Answer 12

the isotopic mass of an isotope relative to 1/12 the mean mass of the C-12 isotope

Question 13

what is relative molecular mass

Answer 13

mean mass of a molecule of a compound relative to 1/12 the mean mass of the C-12 isotope

Question 14

what is relative formula mass

Answer 14

Mr but used for compounds with giant structures

Question 15

how are ions formed

Answer 15

when an atom gains or looses an electron

Question 16

what are they used for

Answer 16

the analytical technique of mass spectrometry

Question 17

what is time of flight

Answer 17

time of flight records the time it takes for ions of each isotope to reach a detector

Question 18

what is step 1 of mass spectrometry

Answer 18

ionisation

Question 19

how is step 1 of mass spectrometry done

Answer 19

atom in gaseous state is bombarded with electrons

Question 20

what is step 2 of mass spectrometry

Answer 20

acceleration

Question 21

how is step 2 of mass spectrometry done

Answer 21

positively charged ions are accelerated to a negative detector

Question 22

what is step 3 of mass spectrometry

Answer 22

ion drift

Question 23

how is step 3 done

Answer 23

ions are deflected by a magnetic field into a curved path

Question 24

what is step 4 of mass spectrometry

Answer 24

detection

Question 25

how is step 4 of mass spectrometry done

Answer 25

+ ions git the - detection plate. they gain an electron, producing a current. the greater the abundance, the greater the current produced

Question 26

what is step 5 of mass spectrometry

Answer 26

analysis

Question 27

how is step 5 of mass spectrometry done

Answer 27

current values are used in a combination with the flight times

Question 28

how can u calculate the Ar using printed spectra

Answer 28

Ar-(m/z x abundance)/ total abundance

Question 29

what is ionisation energy

Answer 29

the minimum energy required to remove the highest energy electron from an atom in its gaseous state

Question 30

what is successive ionisation energies

Answer 30

when further electrons are removed- usually requires more energy because as electrons are removed, the electrostatic forces increase between the nucleus and electrons

Question 31

trend in 1st ionisation across a period

Answer 31

increases as the radius decreases due to more electrons and more electrostatic forces

Question 32

trend in 1st ionisation down a group

Answer 32

decreases as there are more shells that act as shielding and therefore there are less electrostatic forces

Question 33

what does a sudden large increase in successive ionisation energies on a graph indicate

Answer 33

a change in energy levels

Question 34

why is the first ionisation energy of aluminium lower than expected?

Answer 34

it has a single pair of electrons with opposite spin. this means there is a repulsion

Question 35

what is the current model of electronic configuration based on

Answer 35

- emmission spectra provides evidence for quantum shells - successive ionisation energies prove quantum shells within atoms and sugest the atoms group - first ionisation energy

Question 36

what are electron orbitals

Answer 36

a cloud of negative charge where electrons are held

Question 37

what are the different types of electron orbitals

Answer 37

S P D & F

Question 38

what is the shape os the S orbital

Answer 38

spherical

Question 39

what is the shape of the P orbital

Answer 39

dumbbell

Question 40

what do the electron orbitals corrispond with

Answer 40

blocks in the periodic table

Question 41

what periods fall in the S block

Answer 41

periods 1&2

Question 42

what periods fall in the D block

Answer 42

Transition metals

Question 43

what periods fall in the P block

Answer 43

3,4,5,6,7&8

Question 44

what periods fall in the F block

Answer 44

the two at the bottom

Question 45

how many electrons can the S subshell hold

Answer 45

2 electrons

Question 46

how many electrons can the P subshell hold

Answer 46

6 electrons

Question 47

how many electrons can the D subshell hold

Answer 47

10 electrons

Question 48

what is the energy trend of the orbitals from S-D

Answer 48

the energy of the orbitals increase which means that the orbitals are filled from S-D

Question 49

whats the order of the orbitals being filled

Answer 49

S P D F

Question 50

sodium has 11 electrons . how will the configuration be written

Answer 50

Na=1s2, 2s2, 2p6,3s1

Question 51

how many energy levels does sodium have

Answer 51

3

Question 52

how many orbitals does sodium have?

Answer 52

4

Question 53

what is spin in an electron

Answer 53

within an orbital, electrons pair up with opposite spin

Question 54

why do electrons pair up with opposite spin?

Answer 54

so the atom has maximum stability

Question 55

how is spin represented

Answer 55

opposite arrows

Question 56

rule one for writing out electron configurations

Answer 56

the lowest energy orbital is filled first

Question 57

rule two for writing out electron configuration

Answer 57

electrons with the same spin fill up an orbital first before pairing begins

Question 58

what is rule 3 for electron configuration

Answer 58

no single orbital holds more than 2 electrons

Question 59

what is an exception to the rule?

Answer 59

if electron spins are unpaired and therefore unbalanced, it produces a natural repulsion between the electrons

Question 60

what does a natural repulsion within the electrons result in

Answer 60

a very unstable atom

Question 61

what happens when the atom is unstable

Answer 61

the electrons may take a different arrangement to improve stability

Question 62

the 3p4 orbital has a single pair of electrons with opposite spins making it unstable, what then happens

Answer 62

an electron moves to the 4s shell to make it more stable and the configuration is now 3p3 4s1

Question 63

what does periodicity refer to

Answer 63

the study of patterns of physical atomic and chemical properties

Question 64

what does the periodic table arrange the elements by

Answer 64

the atomic (proton) number

Question 65

what do the elements along a period have in common

Answer 65

they have the same number of shells

Question 66

what do elements down a group have in common?

Answer 66

they have the same umber of electrons in its outer shell

Question 67

what happens to the atomic radius across a period and why

Answer 67

decreases because there are more electrons which means there is a higher nuclear charge and more inter molecular forces

Question 68

what happens to atomic radius down a group and why

Answer 68

increases because there are more shells

Question 69

ionisation energy along a period

Answer 69

increases because of the decreased atomic radius which results in higher attractions

Question 70

ionisation energy down a group

Answer 70

decreases because of more shells which act as sheilds and higher atomic radius

Question 71

where do the melting points of period 2 element peak

Answer 71

around the middle

Question 72

boron and carbon form what?

Answer 72

giant covalent lattices with strong covalent bonds

Question 73

what bonding does lithium and beryllium have?

Answer 73

metallic bonding

Question 74

what is the general trend in ionisation energies along period 2

Answer 74

it increases because the atomic radius is decreasing