unit 2

fuck ch301

Li +

Lithium ion

Na +

sodium ion

K +

potassium ion

NH4 +

ammonium ion

Ag +

silver ion

Mg 2+

Magnesium ion

Ca 2+

Calcium ion

Ba 2+

barium ion

Cd 2+

Cadmium ion

Zn 2+

Zinc ion

Cu +

copper (I) ion aka cuprous

Cu 2+

copper (II) ion aka cupric

Hg2 1+

mercury (i) ion

Hg2 2+

mercury (II) ion

Mn 2+

Manganese (II) ion

Co 2+

cobalt (II) ion

Ni 2+

nickel (II) ion

Pb 2+

lead (II). ion

Sn 2+

tin (II) ion aka stannous

Sn 4+

tin (IV) ion (stannic)

Fe 2+

ion (II) ion (ferrous)

Fe 3+

iron (III) ion aka ferric

Al 3+

aluminum ion

Cr 3+

chromium (III) ion

F-

fluoride ion

Cl -

Chloride ion

Br -

bromide ion

I -

iodide ion

OH-

hydroxide ion

CN-

cyanide ion

ClO-

hypochlorite ion

ClO2 -

chlorite ion

Cl03 -

chlorate ion

Cl04 -

perchlorate

CH3COO-

acetate ion

C2O4 2-

oxalate ion

MnO4 -

permanganate

NO2 -

nitrite ion

NO3 -

nitrate ion

SCN -

thicyanate

CN -

cyanide

OCN -

cyanate

N 3-

nitride

O 2-

oxide ion

S 2-

sulfide ion

HSO3 -

bisulfite ion

HSO4 -

bisulfate ion

HSO4 -

bisulfate ion

SO4 2-

sulfate ion

PO4 3-

phosphate ion

HCO3-

bicarbonate

CO3 2-

carbonate ion

CrO4 2-

chromate ion

Cr2O7 2-

dichromate ion

representative elements

group a; assigned to s or p orbital

d-transition

group b; assigned to a d orbital

f-transition (inner transition orbitals)

assigned to f orbtial

effective nuclear charge

net nuclear charge after taking into consideration shielding

\
always less than Zactual

atomic radii

size of atom

ionic radius

the size of an atom compared to an ion of the same element

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smallest to largest is cation → neutral → anion

first ionization energy

HINT: nazi wanted to remove jews → niza remove

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the minimum amount of energy required to remove the most loosely held electron from an isolated atom in the gas phase

\
EXCEPTIONS: group III and IV due to their electron configurations having full pairs except for one

second ionization energy

energy required to remove second electron

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ALWAYS greater than the first ionization energy due to the fact that removing an electron from a cation is considerably more difficult since the electrons are most tightly bounded

electron affinity

energy associated when an electron is added to an atom in the gas phase

electronegativity

the ability for an atom is hold an electron tightly to the nucleus

isolelectronic

elements and ions that have the same electron configuration and number of electrons

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size will go from low atomic # → higher atomic #

(higher atomic # will have more protons, therefore holding the electrons tighter to the nucleus)

exception when losing electrons for transition metals

lose (n-1)d orbitals before ns

forming a bond

energy released

\
exothermic

\
E < 0

breaking a bond

energy absorbed

\
endothermic

\
E > 0

lattice energy

energy released from the formation of gas phase elements to a crystallic state (a lattice strcture)…REMEMBER FORMING BOND → ENERGY RELEASED

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uses Coulomb’s law

heat of formation

energy released from the formation of bond from its NATURAL state

diatomic molecules

**H**ave

**N**o

**F**ear

**O**f

**I**ce

**C**old

__**B**____ee__**r**

melting point

correlates with lattice energy

ionic bond

formed through the electrostatic attraction between ions

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TRANSFERRED from one species to another

\
want to achieve noble gas configuration

\
usually formed when the electronegativity difference is large

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metal + nonmetal (metal more IE and nonmetal more EA)

formula unit

ionic compound with ions in lowest ratio

covalent bond

compound formed through the sharing of electrons

\
formed between nonmetals (similar EN)

ionic compound

solids at room temp

ionic compound

>400 degrees C

ionic compound

insoluble in non-polar solvents

ionic compound

good conductor in molten and aqueous

ionic compound

network of cations and anions held by electrostatic forces

covalent compound

can be solid, liquid, or gases

covalent compound

covalent compound

soluble in non-polar solvents

covalent compound

not good conductors in any state (due to the fact that there are no charges in the compound)

covalent compound

form individual molecules

bond length

distance between the chemical bonds and indicates stability within a compound

hydrogen

needs 2 e- to achieve stable state

beryllium

needs 4 e- to achieve a stable state

boron

needs 6- to achieve a stable state

aluminum

needs 6- to achieve a stable state

formal charge

atomic # - number of assigned electrons

resonance

same arrangement of atoms but different arrangement of electrons

\
involves delocalized electrons

below 3

can have expanded octet rule

2

0

linear

linear

180 degrees

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

3

0

trigonal planar

trigonal planar

120 degrees

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

3

1

trigonal planar

bent

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

4

0

tetrahedral

tetrahedral

109\.5 degree

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

4

1

tetrahedral

trigonal pyramidal

109\.5 degrees

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

4

2

tetrahedral

bent

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???

5

0

trigonal bipryamidal

90 degrees, 120 degrees

\# of rhed ???

\# of lone pairs ???

electronic geometry ???

molecular geometry ???

bond angle ???