Chemistry Unit 3

- hight melting points (all execpt mercury are solid at room temperature)

- shiny when freshly cut or polished

- malleable (dehnbar) -> can pushed into a sheet

- ductile (plastisch verformbar) -> can be pulled into thin water 

- generally flexible as thin sheets or wires

- good conductors of heat and elctricity

- tend to lose electrons and form positive ions when reacting

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- lower melting points

- solids are not malleable, ductile or flexible

- poor conductors of heat and electricity 

- tend to gain electorns and form negative ions when reacting or will share electrons when reacting with other non-metals

- have a blend of properties of metals and non-metals

- most are partial electrical conductors at room temperature

electrons in the outer most level/shell

the number of valence electrons

it has the name akali metals.

- soft, silvery solids

- the most reactive of all metals

- corrode rapidly in air to a dull gray

- readily form compounds with non-metals, the resulting compounds are highly soluble in water.

- have one valance electron

- lose 1 electron to make ions with one positive charge

- react vigorously with water to produce hydrogen gas

They have the name Alkaline Earth Metals.

- silvery solids, harder than alkali metals

- corrode more slowly in air to a dull gray

- react with water to produce hydrogen gas (not as vigourously as  alkali metals)

- form compounds with non-metals, the resulting compounds often have lower solubility in water

- form compounds with non-metals, the resulting compounds often have lower solubility in water

- have 2 valence electrons

- lose two electrons to make ions with a two charge

They have the name halogens.

- very reactive non-metals with 7 valence electrons

- gain one electron

It has the name noble gases.

- non-reactive, full outer shells

- do not gain or lose electrons

ions and elements with the same electron configuration (these will have the same number of electrons)

the size of an ato from the centre of the nucleus to the outermost energy level

going across a period, atoms have the same number of energy levels but more electrons and protons which increases the attraction between the nucleus and the electrons, causing the outer shell/level to be pulled in and thus the radius decreases

going down a family, each new period represents a new shell added further away from the nucelus, each new energy level increases the radius

energy required (erforderlich) to remove an electron from a neutral atom

the ionization energy, as radius decreases (increasing electron-proton attractiom), ionization energy increases

the ability of an atom to attract a bonding electron

metals tend to lose electrons, non metals tend to gain electrons, elements with a stronger tendency to lose electrons are considered more metallic

- only noble gas atoms have full outer electrons shell, this is the most stable arrangement

- when atoms react, they either lose, gain or share electrons in a way that allows them to have full outer electrons shells, gaining stability

- ionic bond

- pure covalent bonds

- polar covalent bonds

They do it when they have extremely different electronegativity. 

the attraction between oppositely charged ions is called an ionic bond.

They do it when both atoms have high electronegativity, so both atoms want to attract an electron, but neither atom can take electrons from the other atom

a bond created when to atoms which hold their electrons strongely (non-metals) share a pair of electrons. 

if both atoms have very similar electronegativities, electrons are shared equally between atoms creating a bond with no electrical charge

if both atoms have electronegativities that are significantly different but not different enough to create an ionic bond, electrons are shared unequally between the atoms

the more electronegative atom pulls the electrons closer, this atom becomes negative

this create a bond with one slightly negative end and one slightely positive end

these negativee and positive poles make a dipole

a covalent bond with a dipole

yes, it depends on the symmetry