Final Exam Flashcards
Acetate ion
CH3COO^1-
Hydrogen carbonate (bicarbonate) ion
HCO3^1-
Hydroxide ion
OH^1-
Nitrate ion
NO3^1-
Carbonate ion
CO3^2-
Sulfate ion
SO4^2-
Phosphate ion
PO4^3-
Ammonium ion
NH4^1+
Cu
Copper(I) = Cu^1+Copper(II) = Cu^2+
Fe
Iron(II) = Fe^2+Iron(III) = Fe^3+
Pb
Pb^2+ lead(II) ion Pb^4+ lead(IV) ion
Sn
Sn^2+ tin(II) ion Sn^4+ tin(IV) ion
CH3COO^1-
Acetate ion
HCO3^1-
Hydrogen carbonate (bicarbonate) ion
OH^1-
Hydroxide ion
NO3^1-
Nitrate ion
CO3^2-
Carbonate ion
SO4^2-
Sulfate ion
PO4^3-
Phosphate ion
NH4^1+
Ammonium ion
Chemistry
Study of composition of matter and the changes it undergoes
Democritus
Atomos
Aristotle
Continuous view
Scientific method
1700sObservation, hypothesis, experimentation, analyzation
A. Lavoisier
Law of conservation of matter
Law of conservation of matter(mass)
In a chemical reaction matter cannot be created nor destroyed. Only change forms
Law
A brief statement or mathematical equation that summarizes a large amount of results and predicts future results
Theory
Very detailed explanation of what is happening
Sir. F. bacon
Science is the answer. It will solve our problems
Rachel Carson
Wrote silent spring. Led to green chemistry
Green chemistry
Reduce wasteSafer solvents
Physical properties/changes
Characteristics displayed without change in composition. Color, phys state, odor, etc. dissolve. It disperses doesn’t change.
Chemical properties/changes
Rust, fire, inert, chemical reactions
Kinetic energy in states of matter
Solid lowestLiquid middleGas highest
Solid
Particles packed closely together in fixed positions. Incompressible. Independent shape and volume
Liquid
Particles in close contact but freely nice past one anotherIndependent volume
Gas
Particles separate from one another. Large gaps between particles. Compressible Takes shape and volume of container
Adding sig fig
Answer may only have as many decimal places as the original value with the fewest
Multiplying sig fig
Answer may only have as many sig figs as original value with the fewest
Mixtures
Contain 2 or more pure substances not chemically combined. Fairly easy to seperate
Pure substances
Composed of one type of atom or molecule.
Heterogeneous mixture
Uneven distribution of components. Oil &water
Homogenous
Even distribution. SolutionsMilk; soda
Element
Composed of one type of atom
Atom
Smallest part of an element that still has properties of that element
Compound
Composed of two or more types if atoms
Molecule
2 or more atoms chemically bonded together.
Au
Atomic element
O (subscript)2
Molecular element
H2O
Molecular compound
Energy
Ability to do work or cause change
Potential energy
Stored E. E of position. Energy in chem bonds
Kinetic energy
E of motion. Thermal
Law of conservation of energy
Energy is neither created it destroyed
1 cal = J
4.18
Calorie
energy required to raise 1g of water 1C
Boiling freezing absolute zero
Boiling 212 F 100 C 373KFreezing 32F. 0C. 273KAbs Zero -460 F. -273C 0K
J. Proust
Law of definite proportions
Law of definite proportions
Any given compound is always composed of the same elements in the same mass ratio
J. Dalton
Law of multiple proportionsAndAtomic theory
Law of mult proportions
Elements may combine in a variety or ratios but a different compound will result
Mendeleev
Periodic law
Periodic law
When we arrange elements according to their atomic mass their proportions occur periodically
WM crookes
Cathode ray tube
Jj Thomson
Plum pudding model(Discovered electron)
Plum pudding model
Atom composed if positively charged stuff with negatively charged particles randomly embedded
E. Rutherford
Nuclear model
Nuclear model
Atom is mostly empty space. W/dense central nucleus. Inside are positivity charged particles (protons). Electrons outside nucleusStadium peas(elephant) fly
Chadwick
Discovered neutron. Inside nucleus with protons. No charge
Atomic mass number
Sum of protons plus neutrons
Atomic number
Number of protons
Isotope
Same atomic number Diff atomic mass
Bohr
Planetary modelEnergy levels 2nsquared
Valence electrons
Electrons in hugest n levelMost reactive
Group 1A
Alkali metals
Group 2A
Alkaline earth metals
Group 7A
Halogens
Group 8A
Noble gases
Metals on ptable
Left of zig
Non metals on ptable
Right of zig
Metalloid
On zig except Al
Lewis dot structure
Represents valence electrons
Hydrogen
H
Carbon
C
Oxygen
O
Nitrogen
N
Fluorine
F
Sodium
Na
Magnesium
Mg
Aluminum
Al
Phosphorus
P
Sulfur
S
Chlorine
Cl
Potassium
K
Calcium
Ca
Helium
He
Iron
Fe
Copper
Cu
Zinc
Zn
Bromine
Br
Silver
Ag
Iodine
I
Gold
Au
Lead
Pb
Rubidium
Rb
Tin
Sn
Lithium
Li
Neon
Ne
Argon
Ar
Strontium
Sr
H
Hydrogen
C
Carbon
O
Oxygen
N
Nitrogen
F
Fluorine
Na
Sodium
Mg
Magnesium
Al
Aluminum
P
Phosphorus
A
Sulfur
Cl
Chlorine
K
Potassium
Ca
Calcium
He
Helium
Fe
Iron
Cu
Copper
Zn
Zinc
Br
Bromine
Ag
Silver
I
Iodine
Au
Gold
Pb
Lead
Rb
Rubidium
Sn
Tin
Li
Lithium
Ne
Neon
Ar
Argon
Sr
Strontium
isoelectronic
2 species w/same total e-
anion
atom with overall negative charge
cation
atom with overall positive charge
ion
atom that carries an overall charge
metals _______ electrons
loose
Ionic Compound Name
metal nonmetal-ending changed to ide
Poly Atomic Name
end in -ate
What is a Poly Atomic ion?
a charged particle consisting of two or more covalently bonded atoms. They remain together through most chemical reactions
Molecular vs ionic compound
– molecular compounds (covalent) share electrons, and form between two non-metals. Ionic give electrons and form between a metal and nonmetal
Polar vs nonpolar bonds
– different elements = usually polar, same element = nonpolar
Electronegativity
a measure of the attraction of an atom of that element in a molecule for a pair of shared electrons. Atoms on the right of periodic table are more electronegative than those on the left. Atoms at top of a column are generally more electronegative than the bottom.
NaOH
Sodium Hydroxide (POLYATOMIC)
Covalent Compound Prefixes
mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
avogadro’s number
6.022 x 10^23 atoms/molesaka 1 mole
parts of a solution
solute: item in lesser amount. Solvent: Item in greater amount (usually does the dissolving)
Molarity (M)
moles of solute/L of solution
Energy
ability to do work or cause change
Potential E
Energy of position (stored E)
Kinetic E
Energy of Motion
For Chemical reaction to occur:Bond breaking is ________.Bond Formation is ________.
breaking requires input of energy (endothermic)Bond formation releases energy (exothermic)
E of Activation
the amount of energy required for a reaction to occur
catalyst
lowers E of Activation
Entropy
degree of disorder
Energy of Fusion
increase in E input but temp stays the same
(specific) heat capactiy
amount of energy required to raise the temperature of a substance a given amount. i.e. solid to liquid
Acetate ion …
CH3COO^1-
Hydrogen carbonate (bicarbonate) ion
HCO3^1-
Hydroxide ion
OH^1-
Nitrate ion
NO3^1-
Carbonate ion
CO3^2-
Sulfate ion
SO4^2-
Phosphate ion
PO4^3-
Ammonium ion
NH4^1+
Cu
Copper(I) = Cu^1+Copper(II) = Cu^2+
Fe
Iron(II) = Fe^2+Iron(III) = Fe^3+
Pb
Pb^2+ lead(II) ion Pb^4+ lead(IV) ion
Sn
Sn^2+ tin(II) ion Sn^4+ tin(IV) ion
CH3COO^1-
Acetate ion
HCO3^1-
Hydrogen carbonate (bicarbonate) ion
OH^1-
Hydroxide ion
NO3^1-
Nitrate ion
CO3^2-
Carbonate ion
SO4^2-
Sulfate ion
PO4^3-
Phosphate ion
NH4^1+
Ammonium ion
Chemistry
Study of composition of matter and the changes it undergoes
Democritus
Atomos
Aristotle
Continuous view
Scientific method
1700sObservation, hypothesis, experimentation, analyzation
A. Lavoisier
Law of conservation of matter
Law of conservation of matter(mass)
In a chemical reaction matter cannot be created nor destroyed. Only change forms
Law
A brief statement or mathematical equation that summarizes a large amount of results and predicts future results
John Dalton
Atomic theory
Theory
Very detailed explanation of what is happening
Sir. F. bacon
Science is the answer. It will solve our problems
Rachel Carson
Wrote silent spring. Led to green chemistry
Green chemistry
Reduce wasteSafer solvents
Physical properties/changes
Characteristics displayed without change in composition. Color, phys state, odor, etc. dissolve. It disperses doesn’t change.
Chemical properties/changes
Rust, fire, inert, chemical reactions
Kinetic energy in states of matter
Solid lowestLiquid middleGas highest
Solid
Particles packed closely together in fixed positions. Incompressible. Independent shape and volume
Liquid
Particles in close contact but freely nice past one anotherIndependent volume
Gas
Particles separate from one another. Large gaps between particles. Compressible Takes shape and volume of container
Adding sig fig
Answer may only have as many decimal places as the original value with the fewest
Multiplying sig fig
Answer may only have as many sig figs as original value with the fewest
Mixtures
Contain 2 or more pure substances not chemically combined. Fairly easy to seperate
Pure substances
Composed of one type of atom or molecule.
Heterogeneous mixture
Uneven distribution of components. Oil &water
Homogenous
Even distribution. SolutionsMilk; soda
Element
Composed of one type of atom
Atom
Smallest part of an element that still has properties of that element
Compound
Composed of two or more types if atoms
Molecule
2 or more atoms chemically bonded together.
Au
Atomic element
O (subscript)2
Molecular element
H2O
Molecular compound
Energy
Ability to do work or cause change
Potential energy
Stored E. E of position. Energy in chem bonds
Kinetic energy
E of motion. Thermal
Law of conservation of energy
Energy is neither created it destroyed
1 cal = J
4.18
Calorie
energy required to raise 1g of water 1C
Boiling freezing absolute zero
Boiling 212 F 100 C 373KFreezing 32F. 0C. 273KAbs Zero -460 F. -273C 0K
J. Proust
Law of definite proportions
Law of definite proportions
Any given compound is always composed of the same elements in the same mass ratio
J. Dalton
Law of multiple proportionsAndAtomic theory
Law of mult proportions
Elements may combine in a variety or ratios but a different compound will result
Mendeleev
Periodic law
Periodic law
When we arrange elements according to their atomic mass their proportions occur periodically
WM crookes
Cathode ray tube
Jj Thomson
Plum pudding model(Discovered electron)
Plum pudding model
Atom composed if positively charged stuff with negatively charged particles randomly embedded
E. Rutherford
Nuclear model
Nuclear model
Atom is mostly empty space. W/dense central nucleus. Inside are positivity charged particles (protons). Electrons outside nucleusStadium peas(elephant) fly
Chadwick
Discovered neutron. Inside nucleus with protons. No charge
Atomic mass number
Sum of protons plus neutrons
Atomic number
Number of protons
Isotope
Same atomic number Diff atomic mass
Bohr
Planetary modelEnergy levels 2nsquared
Valence electrons
Electrons in hugest n levelMost reactive
Group 1A
Alkali metals
Group 2A
Alkaline earth metals
Group 7A
Halogens
Group 8A
Noble gases
Metals on ptable
Left of zig
Non metals on ptable
Right of zig
Metalloid
On zig except Al
Lewis dot structure
Represents valence electrons
Hydrogen
H
Carbon
C
Oxygen
O
Nitrogen
N
Fluorine
F
Sodium
Na
Magnesium
Mg
Aluminum
Al
Phosphorus
P
Sulfur
A
Chlorine
Cl
Potassium
K
Calcium
Ca
Helium
He
Iron
Fe
Copper
Cu
Zinc
Zn
Bromine
Br
Silver
Ag
Iodine
I
Gold
Au
Lead
Pb
Rubidium
Rb
Tin
Sn
Lithium
Li
Neon
Ne
Argon
Ar
Strontium
Sr
H
Hydrogen
C
Carbon
O
Oxygen
N
Nitrogen
F
Fluorine
Na
Sodium
Mg
Magnesium
Al
Aluminum
P
Phosphorus
A
Sulfur
Cl
Chlorine
K
Potassium
Ca
Calcium
He
Helium
Fe
Iron
Cu
Copper
Zn
Zinc
Br
Bromine
Ag
Silver
I
Iodine
Au
Gold
Pb
Lead
Rb
Rubidium
Sn
Tin
Li
Lithium
Ne
Neon
Ar
Argon
Sr
Strontium
Meth
1
Eth
2
Prop
3
But
4
Pent
5
Hex
6
Hept
7
Oct
8
Dec
10
Non
Nine
