periodic table

Question 1

how do you tell which element is in which period or group

Answer 1

period: number of orbital shells
group: number of valency electrons

Question 2

group 1 is also known as?

Answer 2

alkali metals

Question 3

what are the physical properties of group 1? (5)

Answer 3

low m&b point, decreases down the group
low density, increases down grp,
soft metals,
good conductor of h&e
malleable and ductile

Question 4

why do elements of group 1 melting and boiling points decreases down the group?

Answer 4

atomic size increases down the grp,
electrostatic force is attraction between metals cations and negative sea of electrons become weaker,
less heat needed to overcome weaker force

Question 5

reason why density increases down the grp 1

Answer 5

mass increases more than volume

Question 6

what is the reason group 1 metals are malleable?

Answer 6

layers of metal cation can slide past each other without breaking when force is applied

Question 7

what are the chemical properties of group 1 (1)

Answer 7

reactive, increases down the group

Question 8

why do elements in the same group have similar chemical reactions?

Answer 8

because they have the same number of valence electron

Question 9

why does the reactivity of group 1 increases down the group?

Answer 9

as you go down, atomic radius becomes bigger
the valence electron is further away from the nucleus
the force of attraction between the valence electron becomes weaker
easier to release/donate valence electron

Question 10

metal reacts with what to from hydrogen

Answer 10

water (metal + water–>metal hydroxide +hydrogen)

Question 11

Metal + oxygen gives you? it dissolves in water to produce?

Answer 11

metal oxide; alkali solution

Question 12

group 1 burns in ______ to from white solid

Answer 12

chlorine

Question 13

which 2 metals does not form white solids compound? and what colour are they?

Answer 13

potassium dichromate VI - orange and potassium manganate VII - purple

Question 14

group 8 is also known as?

Answer 14

noble/ inert gases

Question 15

what are the 5 physical properties of group 8?

Answer 15

low density, colourless, insoluble in water, poor conductor of heat and electricity, low melting point

Question 16

why are group 8 elements a poor conductor of heat and electricity?

Answer 16

they do not have free moving electrons or ions to carry the electrical charge

Question 17

why do group 8 elements hv increasing melting and boiling points down the grp?

Answer 17

the atomic size gets bigger, therefore there are more forcers of attraction between the atoms, thus more energy is needed to overcome the stronger force.

Question 18

2 chemical properties of grp8 are?

Answer 18

chemically unreactive and are monoatomic gases at room temp and pressure

Question 19

uses of helium, neon, argon, krypton , xenon?

Answer 19

balloons, signs ,electrical bulbs, electrical devices and lasers, electricals flash guns

Question 20

group 7 is known as?

Answer 20

halogens

Question 21

idk name the 3 general things abt grp 7????

Answer 21

diatomic, form salt when reacting with most metal and posinous

Question 22

physical properties of group 7? (5)

Answer 22

low melting point, low density, colours get darker, soluble in water and poor conductor of heat and electricity

Question 23

what is the reason group 7 have increasing low melting and boiling points down the group

Answer 23

the atomic size gets bigger, forces of attraction between molecules are stronger, more heat needed to overcome

Question 24

colours and state of metals of grp 7 elements? f,cl,br,i,at

Answer 24

pale yellow, yellow- green gas, orange brown liquid, purple solid, black solid

Question 25

solubility of grp 7

Answer 25

easily soluble, very soluble, partially soluble, insoluble, insoluble

Question 26

chemical properties of grp 7 (1)

Answer 26

reactivity decreases down the grp

Question 27

why does reactivity decrease down group 7

Answer 27

atomic size increases down the grp, outermost shell is further away from nucleus, FOA between nucleus and outer most shell is weaker, harder to gain electrons from other atoms

Question 28

why are grp 7 so reactive?

Answer 28

because they hv the tendency to accept electrons to make a stabel full outer shell

Question 29

grp 7 reacts with water to from

Answer 29

2 acids, one of which are bleaching property

Question 30

grp 7 reacts with hot iron to from ?

Answer 30

brown solid, iron III halides

Question 31

how does displacement react with grp 7 idk man

Answer 31

more electronegative halogen can displace a less electronegative

Question 32

physical properties of transitional metals (7)

Answer 32

hard, malleable and ductile, high melting and boiling and density, high tensile strength , conduct H&E, shiny surface,

Question 33

what are the chemical properties of transitional metals (3)

Answer 33

catalytic properties, forms coloured compounds and ions in solute, variable oxidisation state,

Question 34

does the atomic sizes decrease or increase across the period 3? why

Answer 34

decreases; proton number increase by 1 unit to the next so the positive charge increases, nuclei attraction on orbital shells containing electrons increasers and the orbital shells are pulled inwards

Question 35

electronegativity increases across periodic 3 because?

Answer 35

atomic size decreases but the positive charge increases. strength of atoms attract electrons increases
remeber: electronegativity is the strength to attracts electrons

Question 36

name the types of oxide for
MgO, P4O10, Al2O3, SiO2, Cl2O7, Na2O, SO2

Answer 36

basic, acidic, amphoteric, acidic, acidic, basic, acidic

Question 37

meaning of valency

Answer 37

number of electrons its atoms lose, gain or share to form a compound

Question 38

why does reactivity decreases down the grp ?

Answer 38

more electrons a metal needs to lose, the more difficult

Question 39

why does reactivity increases across non-metals?

Answer 39

fewer electrons a non-metal needs to gain, easier to attract them