periodic table Flashcards
how do you tell which element is in which period or group
period: number of orbital shells
group: number of valency electrons
group 1 is also known as?
alkali metals
what are the physical properties of group 1? (5)
low m&b point, decreases down the group
low density, increases down grp,
soft metals,
good conductor of h&e
malleable and ductile
why do elements of group 1 melting and boiling points decreases down the group?
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
reason why density increases down the grp 1
mass increases more than volume
what is the reason group 1 metals are malleable?
layers of metal cation can slide past each other without breaking when force is applied
what are the chemical properties of group 1 (1)
reactive, increases down the group
why do elements in the same group have similar chemical reactions?
because they have the same number of valence electron
why does the reactivity of group 1 increases down the group?
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
metal reacts with what to from hydrogen
water (metal + water–>metal hydroxide +hydrogen)
Metal + oxygen gives you? it dissolves in water to produce?
metal oxide; alkali solution
group 1 burns in ______ to from white solid
chlorine
which 2 metals does not form white solids compound? and what colour are they?
potassium dichromate VI - orange and potassium manganate VII - purple
group 8 is also known as?
noble/ inert gases
what are the 5 physical properties of group 8?
low density, colourless, insoluble in water, poor conductor of heat and electricity, low melting point
why are group 8 elements a poor conductor of heat and electricity?
they do not have free moving electrons or ions to carry the electrical charge
why do group 8 elements hv increasing melting and boiling points down the grp?
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.
2 chemical properties of grp8 are?
chemically unreactive and are monoatomic gases at room temp and pressure
uses of helium, neon, argon, krypton , xenon?
balloons, signs ,electrical bulbs, electrical devices and lasers, electricals flash guns
group 7 is known as?
halogens
idk name the 3 general things abt grp 7????
diatomic, form salt when reacting with most metal and posinous
physical properties of group 7? (5)
low melting point, low density, colours get darker, soluble in water and poor conductor of heat and electricity
what is the reason group 7 have increasing low melting and boiling points down the group
the atomic size gets bigger, forces of attraction between molecules are stronger, more heat needed to overcome
colours and state of metals of grp 7 elements? f,cl,br,i,at
pale yellow, yellow- green gas, orange brown liquid, purple solid, black solid
solubility of grp 7
easily soluble, very soluble, partially soluble, insoluble, insoluble
chemical properties of grp 7 (1)
reactivity decreases down the grp
why does reactivity decrease down group 7
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
why are grp 7 so reactive?
because they hv the tendency to accept electrons to make a stabel full outer shell
grp 7 reacts with water to from
2 acids, one of which are bleaching property
grp 7 reacts with hot iron to from ?
brown solid, iron III halides
how does displacement react with grp 7 idk man
more electronegative halogen can displace a less electronegative
physical properties of transitional metals (7)
hard, malleable and ductile, high melting and boiling and density, high tensile strength , conduct H&E, shiny surface,
what are the chemical properties of transitional metals (3)
catalytic properties, forms coloured compounds and ions in solute, variable oxidisation state,
does the atomic sizes decrease or increase across the period 3? why
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
electronegativity increases across periodic 3 because?
atomic size decreases but the positive charge increases. strength of atoms attract electrons increases
remeber: electronegativity is the strength to attracts electrons
name the types of oxide for
MgO, P4O10, Al2O3, SiO2, Cl2O7, Na2O, SO2
basic, acidic, amphoteric, acidic, acidic, basic, acidic
meaning of valency
number of electrons its atoms lose, gain or share to form a compound
why does reactivity decreases down the grp ?
more electrons a metal needs to lose, the more difficult
why does reactivity increases across non-metals?
fewer electrons a non-metal needs to gain, easier to attract them
