Elements of life Flashcards by Leah Harman

what is the bonding and structure of each group in the periodic table

1-3=metallic
4-7=covalent

1-4=giant
5-7=molecular

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how have shells of electrons of electrons been proven to exist

atoms produce emission spectra

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what does an atomic emission spectrum look like

coloured lines on a black background

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what does an atomic absorption spectrum look like

black lines on a coloured background

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what does the atomic number of an element tell you about it

number of protons

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what is special about P orbitals

P subshells always contain 3 P orbitals
shells 2 upward contain P orbitals
P orbitals are shaped like a figure of 8

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NO3-

Nitrate

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SO4 2-

sulfate

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CO3

carbonate

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OH-

hydroxide

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NH4

ammonium

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HCO3

hydrogen carbonate

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how many sets do double bonds count for

one

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how does an emission spectrum occur

electrons excited to a higher energy level by heating

- when they fall back down, they emit light

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why is the bond angle of water 104.5degrees

4 sets of electrons with two lone pairs

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how many electrons can a D subshell hold

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what bond is between 2 non-metals

covalent

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what is the equation that links moles, mass and relative atomic mass

mass=molesXrelative atomicmass

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what is special about the S orbitals

spherical

- found in every shell

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which two elements have the same atomic emission spectra

none. all elements have unique energy levels

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on an a-level periodic table what shows you the mass of one mole

relative atomic mass

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what is a dative covalent bond

shared pair electrons

- both electrons come from the same atom

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what is the bond angle and shape of an atom with 4 sets of electrons

109.5

tetrahedral

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how do you predict the amount of a product in a reaction

1-work out moles of known substance 2-work out mole of unknown substance using mole ratio 3.work out mass of unknown substance, m=nXAr

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what bond is between a metal and non metal

ionic

Cu2+

copper

Zn2+

zinc

Pb2+

lead

Fe2+

iron(II)

Fe3+

iron(III)

how do you calculate the % yield

%yield=(actual amount of product-divide- expected amount of product)X100

what is the bond angle and shape of an atom with 3 sets of electrons

120degrees planar

how much does each lone pair reduce the angle by

2.5 degrees

in what order do the subshells fill up in

s, p, d, f

why does nuclear fusion require a high temperature

to overcome the repulsion of the nuclei

what is the empirical formula

simplist ratio of atoms in the compound

what is the equation that links: speed of light, wavelength, frequency

speed of light= wavelength x frequency

what is the bond angle and shape of an atom with 2 sets of electrons

180 linear

why does 4s fill up before the 3d subshell

because it has a lower energy level

what is an orbital

- a 95% probability surface of finding an electron | - 95% of the time an electron will be found in a particular region of the orbital

what is bonding between: calcium oxide, magnesium, carbon dioxide, silicon

ionic metallic covalent covalent

what is the equation that links: planks constant, frequency, energy gap

Energy gap= frequency X planks constant

what is a precipitation reaction

happens when two solutions react together and form an insoluble solid, which is called a precipitate

give 3 key points of ionic bonding

- ionic bonds are strong so have a high melting points | - they do not not conduct electricity as solids

HCO3- NO3- CO3 2- SO4 2-

hydrogen carbonate nitrate carbonate sulfate

HCO3- NO3- CO3 2- SO4 2-

what is the melting point of ionic bonding

ionic bonds are strong. so ionic bonds have high melting point

what is the melting point of metallic bonding

strong attractions between metal ions and delocalised electrons therefore melting point is high

what is the melting point of giant covalent networks

lots of strong covalent bonds therefore high melting points

what is the conductivity of ionic bonding

- do not conduct as solids because ions cannot move | - conduct as solutions and liquids because ions can move

what is the conductivity of metallic bonding

delocalised electrons are free to move, so metals conduct electricity

what is the conductivity of giant covalent networks

only conducts if it contains delocalised electrons

what is the trend in first ionisation energy down group 1

decreases

what is the trend in first ionisation energy across period 3

increases

what is ionisation energy

energy required to remove one electron from each atom in a mole of gaseos atoms

what are some notes on ionisation energy

- looses one electron at a time - electrons need energy to be excited to a very high energy level and leave - removal of electron from outer shell - results in positive ion=more protons than neutrons

what is the first ionisation energy of Na

Na(g)= Na+(g) + e- | first ionisation energy of sodium = +494KJmol-1

what happens with the ionisation energy when you down a group

I.E decreases as the atoms get larger and there is more shielding

in group 1, which element has the highest first I.E

which element has greater shielding-Na or K

K- has more shielding

what is the test for halide ions

add silver nitrate

Elements of life Flashcards

(61 cards)