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TRANSCRIPT
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Valence electrons› electrons in the highest occupied energy level › always in the s and p orbitals
normally just a draw a circle to represent these two orbitals
› determines the chemical properties of an element› usually the only electrons used in chemical bonds
http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_09/FG09_27-06un.JPG
IB may group levels together and therefore you would see the 3d10 before
the 4s2
IB uses this one
electron dot structures/diagrams are used to show valence electrons› each dot around the element symbol represents a
valence electron
B is 1s2 2s2 2p1;› 2 is the outermost energy level › it contains 3 valence electrons, 2 in the
s and 1 in the p Br is [Ar] 4s2 3d10 4p5
How many valence electrons are present?
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when forming compounds, atoms tend to achieve the electron configuration of a noble gas (ns2np6)› this means their highest energy level will be filled
with 8 electrons that requires the least amount of energy
› cations atoms of metallic elements (groups 1-14) lose
electrons producing cations (positive ions) the term oxidized (O.I.L – Oxidized Is Losing) is used
to say it lost an electron example- Ca becomes Ca2+
› anions atoms of nonmetallic elements (groups 15,
16, 17) gain electrons producing anions (negative ions) the term reduced (R.I.G.) – Reduction Is
Gaining) is used to say it gained an electron example- Cl becomes Cl1-
NeNeNNNaNa FF
NaNa+
OO
OO2-
MgMg
MgMg2+
Cations
Anions
NN3- FF1-
...etc.
As it turns out, atoms bond together for a very simple reason: atoms that
have full valence shells are more stable than those that don’t‘.
1+ 2+ 3-3+ 4+/- 2- 1- 0
› some transitional metals can often form more than one cation and therefore charges may vary
some orbitals get filled but might not get a noble gas electron configuration
iron can be Fe2+ or Fe3+ (you don’t have to memorize this)
these always have the same charge Sc3+, Zn2+, Cd2+, Ag1+ (you do have to memorize these)
usually composed oppositely charged metallic cations and nonmetallic anions
› because of the electrostatic attraction between oppositely charged particles electro- electricity/electrons static- non-moving (vs. current which is moving charges)
+ cations
- anions
forms a compound with overall zero charge› (+ and -) need to cancel out
referred to as formula units, not a molecule, that is a term used only for covalently bonds which is something different
ions must have a difference in electronegativity of 1.7 or greater to form an ionic bond
0.1 – 1.0
1.1 – 1.7
>1.7
0.0 covalent, nonpolar
covalent, slightly polar
covalent, very polar
ionic
electronegativtydifference
probable type of bond
Na “gives” Cl one electron and now both atoms have a full valence shell (electron configuration of a noble gas)
3.9
Na Cl
e–1) 2)
3)
Na+ Cl–
shows the kinds and numbers of atoms in the lowest whole-number ratio of ions in the ionic compound› Na 1+ + Cl 1- NaCl
› Ca 2+ + Cl 1- CaCl2
› Mg 2+ + O 2- MgO
Mg and N? Mg2+, N3-
it takes two nitrogens to combine with three magnesiums› Mg3N2
› magnesium nitride
Na 1+ + F 1- NaF
high melting and boiling points › takes a lot of energy to break apart the electrostatic
forces between cations and anions
crystalline structure› repeating arrays of cations and ions› an ionic lattice
volatility- how easily a substance turns into a gas› very low as electrostatic forces between cations
and anions is very strong
electrical conductivity› can conduct electric currents when melted or dissolved
in water because cations and anions are free moving instead in a lattice
solubility› will dissolve in other polar solvents such as water
cations lose valence electrons and therefore are positively charged› transition metals form more than one cation
with different ionic charges› charge is determined from the # of electrons
lost Fe2+ lost two electrons (the 2 in the 4s) Fe3+ lost three electrons (the 2 in the 4s and 1 in the 3d)
› naming Stock system
a Roman numeral is used to show the charge of the transition metal Fe2+ is iron(II) and Fe+3 is iron(III)
Naming Ions
› anions gain valence electrons and therefore are negatively charged change ending to –ide for the name
composed of more than one atom that form a single unit/ion with a charge› most end with -ite or –ate
the –ite ending indicates one less oxygen than the –ate ending ionic charge is the same for both
Memorize these!NO3
-1 nitrate
NO2-1 nitrite
OH-1 hydroxide
ClO2-1 chlorite
ClO3-1 chlorate
HCO3-1 hydrogencarbonat
e (bicarbonate)
SO42- sulfate
SO32- sulfite
CO3 2- carbonate
PO43- phosphate
NH4+ ammonium
Binary Compounds› cation is written first, followed by the anion
with and –ide ending Cs2O cesium oxide
SrF2 strontium fluoride
CuO copper(II) oxide oxygen is always 2- and therefore copper will be 2+
Cu2O copper(I) oxide oxygen is 2- and therefore needed two copper atoms
with 1+ charge
› SnF2 ? fluorine is always 1- and therefore tin
will be 2+
tin(II) fluoride
› SnS2 ? sulfur is always 2- and therefore tin
will be 4+
tin(IV) sulfide
write symbol of cation and then anion add subscripts to balance the charges
› calcium bromide Ca2+ and Br1- is CaBr2
› potassium sulfide K+1 and S2- is K2S
› iron(III) oxide Fe+3 and O2- is Fe2O3
the ionic charge number of each ion is crossed over and becomes the subscript for the other ion
Fe(NO3)3
Choose the correct name for the compound
1. Iron trinitrate
2. iron(I) nitrate
3. iron(III) nitrite
4. iron(III) nitrate
5. none of the abovenext
problemPolyatomic
IonsPeriodic Chart
sodium chlorite
Choose the correct formula for the compound
1. NaCl
2. NaClO
3. NaClO2
4. Na(ClO)2
5. none of the above
next problem
PrefixesPeriodic Chart