module 3- periodic table and energy

Question 1

how many elements when Mendeleev arranged the pt

Answer 1

60

Question 2

Mendeleev arranged the table by …

Answer 2

in order of atomic mass

Question 3

what did Mendeleev do that was special

Answer 3

left spaces for undiscovered elements

Question 4

when were protons discovered

Answer 4

(1900)

Question 5

Ekasilicon - undiscovered element

Answer 5

found in (1886) and named germanium

Question 6

(2014) - the period table has …

Answer 6

-114 elements
- 7 horizontal periods
- 18 groups

Question 7

how is the pt arranged

Answer 7

in order of increasing atomic number, each succesive element has an extra proton

Question 8

groups

Answer 8

the elements are arranged in vertical columns called groups, each element in a group has atoms with the same number of outer shell electron and similar properties

Question 9

periods

Answer 9

horizontal rows - number of highest energy electrons hell in an elements atom

Question 10

periodicity properties

Answer 10

• Electron configuration
• Ionisation energy
• Structure
• Melting points

Question 11

chemistry is determined by

Answer 11

electronic configuration - particularly the outer, highest energy electron shell

Question 12

trends across a period

Answer 12

each period starts with a new electron in its new highest energy shell

Question 13

across p2

Answer 13

the 2nd subshell fills with 2 electrons, followed by the 2p subshell with six electrons

Question 14

across p3

Answer 14

the same pattern of filling shells as 2 is repeated for the 3s and 3p subshells

Question 15

across p4

Answer 15

although the 3d subshell is involved, the highest shell number is n=4, only the 4s and 4p shells are occupied

Question 16

trends-group

Answer 16

Elements in each group have atoms with the same amount of electrons in their outer shell. Elements in the same group also have atoms with the same number of electrons in the subshells - gives the elements the similar chemistry

Question 17

blocks of the periodic table

Answer 17

s,p,d,f

Question 18

new periodic table column numbers

Answer 18

1-18

Question 19

group 1 name

Answer 19

alkali metals

Question 20

group 1 elements

Answer 20

Li,Na,K,Rb,Cs,Fr

Question 21

group 2 name

Answer 21

alkaline earth metals

Question 22

group 2 elements

Answer 22

Be,Mg,Ca,Sr,Ba,Ra

Question 23

group 3-12 name

Answer 23

transition elements

Question 24

group 15/5 name

Answer 24

pnictogens

Question 25

group 15/5 elements

Answer 25

N,P,As,Sb,Bi

Question 26

group 16/6 name

Answer 26

chalcogens

Question 27

group 16/6 elements

Answer 27

O,S,Se,Te,Po

Question 28

group 17/7 name

Answer 28

halogens

Question 29

group 17/7 elements

Answer 29

F,Cl,Br,I,At

Question 30

group 18/0 name

Answer 30

noble gases

Question 31

group 18/0 elements

Answer 31

He,Ne,Ar,Kr,Xe,Rn

Question 32

ionisation energy

Answer 32

ionisation energy measures how easily an atom loses electrons to form positive ions .

Question 33

first ionisation energy

Answer 33

The first ionisation energy is the energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions.

Question 34

example of first ionisation energy

Answer 34

Na(g) → Na+(g) + e-

Question 35

factors affecting ionisation energy

Answer 35

atomic radius, nuclear charge, electron shielding

Question 36

how are electrons held in their shells

Answer 36

Electrons are held in their shells by attraction from the nucleus. The first electron lost will be in the highest energy level and will experience the least attraction from the nucleus.

Question 37

ionisation energy - atomic radius

Answer 37

the greater the distance between the nucleus and the outer electrons, the less the nuclear attraction . the force of attraction falls off sharply with increasing distance, so atomic radius has a large affect

Question 38

ionisation energy- nuclear charge

Answer 38

the more protons there are in the nucleus of an atom, the greater the attraction between the nucleus and the outer electrons

Question 39

ionisation energy - electrons shielding

Answer 39

electrons are negatively charged and so inner shell electrons repel outer shell electrons, reducing the attraction between the nucleus and outer electron shells

Question 40

an element has how many ionisation energies

Answer 40

as many as there are electrons

Question 41

helium ionisation

Question 42

succesive ionisation enegies can be ussed to make prodictions about

Answer 42

• the number of electrons in the outershell
• the group of the element in the periodioc table
• the identity of an element