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Question 1

The main features of the periodic table

Answer 1

1. vertical colunmsare called groups and horixiantal colmums are periods.

2.elemtns are arranged in in the icnreasing order of atomic numbers

4. elements are placed in periods basedon the number of shells in their atoms
5. the shortest period is the period that only contains 2 elements-hydrogenand helium

Question 2

group number in peridoicf table is used to

Answer 2

used to determine the number of valence shells in an atom of an element

Question 3

properties of alkali metals

Answer 3

1. less dense than other metals
   2.only loosely bound electron
2. highly reactive, with reactvitiy increasing moving down the group

4.largest atomic radius of elements in the period

5. low ionisation energy
6. low electronegatviity

Question 4

Alkaline Earth Metals

Answer 4

2 electrons in the valence shell

readily form divalent cations

low electron affinity

low electronegativity.

Question 5

signifance of istopes changing

Answer 5

due to the neutrons changing, the physical properties such density and mass of the atom changes and atomic number, however chemical properties are still very similar.

Question 6

electromagnetic spectrum

Answer 6

th

Question 7

why do we use the bohr model sitll if it snot as accurate

Answer 7

its simpler and easier to understand

Question 8

Electrons in the same shell:

Answer 8

Are about the same distance from the nucleus
Have about the same energy

Question 9

metalloids

Answer 9

a chemical element that exhibits some metal and some nonmetal properties.

Question 10

transition metals

Answer 10

elements that have partially filled d orbitals.

Question 11

halogens

Answer 11

non metals-group 17

itis formed when a salt reacts with a metal

Question 12

noble gas

Answer 12

A gaseous chemical element that has a full shell of valence electrons, and therefore is non reactive.

Question 13

memorise: atomic number
hydrogen,
oxygen,
carbon
nitrogen,
fluroine

Answer 13

hydrogen-1

oxygen-8

carbon-6

nitrogen-7

flurione-9

Question 14

fluroien has a valence shell of 7, why is it less stable then oxygen with a valence shell of 6

Answer 14

fluroine is really close to being a full shell so its more reactiivty than oxygen and therefore very unstable.

Question 15

trends of periodic table

Answer 15

group 1 is alakline,
group 3-12 r transition metalws

Question 16

why are metals very good conductors of elecricty, whereas non metals are bad at it, whilst metalloids rae okay at conducting electircy.

Question 17

non metals tend to gain electrons whereas metals tend to lose electrons

Answer 17

nonmetals gain electrons to have a full shell as they have high electronegativity, whereas metals tned to lose electrons because they have low electrnoegaitvity because they have low ionisation energy.

Question 18

halogen is group

Answer 18

group 17 amd gain electrojn-they exhibit differnet physucal protpeores but same chemical properties

Question 19

physical and chemical properties of halogen

Answer 19

As you go down the halogens, from fluorine to astatine, the elements become darker in colour and have a higher boiling point.

Question 20

noble gases react with

Answer 20

anything unreactive and low electron affinity.

Question 21

how to calculate core charge

Answer 21

the number of proteins in the nucleus - the number of total shells besdies the valence shell

Question 22

electronegavitity

Answer 22

the abilty of an atom to pull electrons from another atom

Question 23

Naturally non metals have

Answer 23

higher electronegatiity

Question 24

Which atoms give up their electrons because they have low electronegatitvty.

Answer 24

metals because they have few valence electrons, they tend to increase theri stabilty by losing electrons to become cations

Question 25

atomic radius

Answer 25

the total distance from the atoms nucleus and valence shell

Question 26

If atomhas high ionsiation energy, it also has

Answer 26

low core charge and low electronegativity

Question 27

fluroine has an atomic radius of 42pm, whereas chlorine has an atomic radius of 175pm, explain the difference

Answer 27

**ask yesh for corrections after trends gone thru

Question 28

Alkali metals properties

Answer 28

1.less dense than other metals

2.
one loosely bound valence electron

3.highly reactive, with reactivity increasing moving down the group

4. largest atomic radius of elements in their period

5.
low ionization energy

6.
low electronegativity

Question 29

properties of transition metals

Answer 29

1.hard, shiny, ductile nad mallebale

2.high melting and boilingpoint

3. high thermal and and electrical conductivity

4,form cations(positive oxidation state)

5. tend to exhibit more than one oxidationstate
6. low ionisation energy

Question 30

properties of metalloids

Answer 30

1.electronegativity and ionization energy between that of metals and nonmetals

2.may possess a metallic luster

3.variable density, hardness, conductivity, and other properties
often make good semiconductors
reactivity depends on nature of other elements in the reaction

Question 31

non metals properties

Answer 31

1.high ionization energy
2.high electronegativity
3.poor electrical and 4.thermal conductors
5.form brittle solids
l6.ittle if any metallic luster
readily gain electrons

Question 32

electron negatiivty, reactivitiy, and valence electrons of halogens

Answer 32

1.extremely high electronegativity

2. very reactive

3.seven valence electrons, so elements from this group typically exhibit a -1 oxidation state

Question 33

The period of an element’s location determines

Answer 33

the number of electronshells

Question 34

core charge

Answer 34

is the measure of the attractive force felt by the valence electrons towards the nucleus.

Question 35

In the periodic table of the elements, the atomic radius tends to increase as you

Answer 35

as you move down a group because the number of electrons is greater, so the circle of electrons in the element gets bigger, making yhe distance betwen the nucleus to the valence shell smaler.

Question 36

The shielding effect

Answer 36

describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. T

Question 37

what atoms expeirence the most sheilding affect

Answer 37

The more electron shells there are, the greater the shielding effect experienced by the outermost electrons.

Question 38

Why does ionisation energy decrease and core charge stays constant when moving down gorups periodic table

Answer 38

the outer electrons are further away from the nucleus and hence aren’t as tightly held

Question 39

Why does ionistiaton energy and core charge increase when moivng left or right across a period

Answer 39

increasing nuclear charge, which results in the outermost electron being more strongly bound to the nucleus.

Question 40

The reactivity of an element is an indication of how

Answer 40

of how easily an atom of that element loses or gains electrons.

Question 41

when metals react thye

Answer 41

they lose electrons

Question 42

Moving down a group, there is an increasing number of e- shells in the atoms, and therefore a

Answer 42

a weaker attractive force betwene the nucleus and the valence shell

and the reactvity ofmetals increase down a group as it is easier for metalswith greater shells to lose electrons

Question 43

why does the reacivity of metals decrease across periods

Answer 43

the reactivity of metals decrease across the periodi as increasing the core charge makes it more difficult for metals to lose electrons

Question 44

what happens to atomic radius across a period

Answer 44

atomic radius decreases, as you move left from right across a period due to increases number of nuclear charge.

Question 45

metallic charcater define

Answer 45

metalliac character is the tendency of an element to lose or gain electrons and form positive ions or cations.

Question 46

metalliac charcater increases and decreases when

Answer 46

metallic character increases as you move down the group because its easier for the element to lose electrons because the atomic radius is increasing.

Question 47

Why does metallic character decrease as you move across periods.

Answer 47

metalliac chracter decreases as you move across periods because the atoms are accepting electrons to fill the shells.

Question 48

what is the link between metallic achacrter and reacivtiity

Question 49

what do metals vs non metals form

Answer 49

metals lose electrons to form cations, whilst non metals gain electrons to form anions