electrons, bonding and structure

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what is first ionisation energy ?
the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
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what 3 factors affect ionisation energy ?
atomic radius , nuclear charge & electron shielding
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what is electron shielding ?
the repulsion between electrons in different inner shells. it reduces net attractive force from the nucleus
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what is successive ionisation energy ?
a measure of the energy required to remove each electron in turn
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why does ionisation energy get larger the more you take away ?
because as each electron is removed there is less repulsion between electrons in each shell , reducing distance from nucleus
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what is the principle quantum number ?
the number representing the electron shell
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what is an atomic orbital ?
a region within an atom that can hold up to two electrons with opposite spins
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what are the 4 types of orbitals ?
s p d & f
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how many electrons can the d sub-shell hold ?
10 electrons
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what is a sub- shell ?
a group of the same type of atomic orbitals within a shell
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why does the 4s sub-shell fill before the 3d ?
because it has a lower energy level
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what is an electron configuration ?
the arrangement of electrons in an atom
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write the electron configuration for sodium (Na) ?
Na: [Ne]3s1
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what are the three types of chemical bonding ?
ionic , covalent & metallic
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what bonds do an metal and non- metal make ?
ionic
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what bonds do 2 non-metals make ?
covalent
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name 2 uses of noble gases ?
helium= airships , Neon= advertising signs , argon= filament light bulbs , krypton= eye surgery lasers
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define an ionic bond ?
the electrostatic attraction between oppositely charged ions
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what charge do metal ions have ?
positive
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what charge do non- metal ions have ?
negative
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what is a giant ionic lattice ?
a 3D structure of oppositely charged particles held together by strong ionic bonds
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what is the formula and charge of ammonium
NH4+
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what is the formula and charge of hydroxide
OH-
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what is the formula and charge of nitrate
NO3-
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what is the formula and charge of nitrite
NO2-
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what is the formula and charge of hydrogen-carbonate
HCO3-
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what is the formula and charge of carbonate
CO3^2-
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what is the formula and charge of sulfate
SO4^2-
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what is the formula and charge of sulfite
SO3^2-
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what is the formula and charge of dichromate
Cr2O7^2-
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what is the formula and charge of phosphate
PO4^3-
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what is a covalent bond ?
a bond formed by a shared pair of electrons
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what is a lone pair ?
an outer- shell pair of electrons that is not involved in chemical bonding
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what is the definition of a dative covalent bond ?
a shared pair of electrons which has been provided by one of the bonding atoms only
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what is expansion of the octet?
when covalent bonding causes more than 8 electrons in the outer shell
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what two rules are slightly more true than the octet ?
unpaired electrons pair up , the maximum electrons that can pair up is equivalent tot he number of electrons in the outer shell
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what is electron repulsion theory ?
the idea that electrons repel each other as far as possible
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on a 3D diagram of bonds , what direction is the shaded wedge going ?
towards you
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whats the name of the shape of a molecule or ion with 2 electron pairs ?
linear
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whats the name of the shape of a molecule or ion with 3 electron pairs?
trigonal planar
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whats the name of the shape of a molecule or ion with 4 electron pairs ?
tetrahedral
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whats the name of the shape of a molecule or ion with 5 pairs of electrons ?
trigonal bipyramid
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whats the name of the shape of a molecule or ion with 6 pairs of electrons ?
octahedral
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whats the name of the shape of a molecule or ion with 2 bonded pairs and 2 lone pairs ?
angular
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whats the name of the shape of a molecule or ion with 2 bonded pairs and 1 lone pair ?
pyramidal
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what are the angles of a linear shape ?
180 degrees
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what are the angles of a trigonal shape ?
120 degrees
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what are the angles of a tetrahedral shape ?
109.5
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what are the angles of a trigonal bipyramid ?
120 horizontal 90 vertical
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what are the angles of a octahedral shape ?
90
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what does a lone pair do to a molecules or ions shape ?
reduces bond angle by 2.5 degrees
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what is electronegativity ?
the measure of an attraction of a bonded atom for the pair of electrons in a covalent bond
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what is a permanent dipole
a small charge difference across a bond that results from a difference in electronegativities of the bonded atoms
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what type of bonds form a permanent dipole ?
polar covalent bonds
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what is a polar molecule ?
a molecule that has an overall dipole when you take into account any dipoles across the bonds
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describe how electronegativity changes on a periodic table
as you go up a group it increases and as you go along a period it also increases
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what is an intermolecular force ?
an attractive force between neighbouring molecules
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name three common types of intermolecular forces ?
hydrogen bonds , permanent dipole-dipole forces and van der waals forces
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what is van der waals force ?
attractive forces between induced dipoles in neighbouring molecules
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what is van der waals forces caused by ?
the movement of electrons in the shells causing an unbalanced charge
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what is a hydrogen bond ?
a strong dipole-dipole attraction between an electron deficient hydrogen atom and a lone pair of electrons
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name three special properties of water
ice is less dense than water , water has a relatively high boiling point , high surface tension.
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what is metallic bonding ?
the electrostatic attraction between positive metal ions and delocalised electrons
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why do giant metallic lattices have high boiling points ?
electrons move through structure , positive ions are in fixed positions, attraction between the two is strong.
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why do giant metallic lattices have good conductivity?
the delocalised electrons move freely, even in solid state
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why are giant metallic lattices malleable and ductile ?
layers can slide past eachother as the electrons can move freely giving a degree of give between layers
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name three properties of ionic compounds ?
high melting and boiling points , can conduct electricity in a solution, soluble in polar solvents
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why cant ionic compounds conduct electricity at a solid state ?
because ions are in fixed positions and so none can move
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why are ionic lattices soluble ?
polar water molecules surround the lattice and break it down .
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what types of structures can covalent compounds have ?
simple molecular , giant covalent
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describe the changes in bonding that occur when i2 changes state?
the weak van der waals forces between the i2 molecules break, however the covalent bonds i-i are strong
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what are 3 properties of simple molecular structures ?
low melting/ boiling points , do not conduct electricity , soluble in non- polar solvents
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name properties of giant covalent structures?
high melting and boiling points , non conductors , non soluble
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Other cards in this set

Card 2

Front

what 3 factors affect ionisation energy ?

Back

atomic radius , nuclear charge & electron shielding

Card 3

Front

what is electron shielding ?

Back

Preview of the front of card 3

Card 4

Front

what is successive ionisation energy ?

Back

Preview of the front of card 4

Card 5

Front

why does ionisation energy get larger the more you take away ?

Back

Preview of the front of card 5
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gurl this is really good...well done :)

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