Chemistry Final Review Flashcards

Chemistry Flashcards for Final Review

What is Chemistry?

The study of matter and the changes it undergoes.

What determines the identity of an element?

The number of protons (atomic number).

What are Isotopes?

Same element, different masses, different number of neutrons.

What is the relationship between energy level and distance from the nucleus?

The larger the energy level, the farther away from the nucleus.

Differentiate between Ground State and Excited State.

Ground State: low energy. Excited State: higher energy.

What happens during the Hydrogen Line Emission Spectrum?

Electrons fall from an excited state to a ground state and release a photon.

What occurs during Absorption?

Atom takes in energy; electron moves to an excited state.

What occurs during Emission?

Atom releases energy; electron falls to ground state.

What are the three different nuclear decay particles?

Alpha, Beta, and Gamma.

Describe Alpha decay particle

Symbol: He, Charge: +2, Mass: 4, Strength: very weak, Blocked by: paper, Attracted to negative

Describe Beta decay particle

Symbol: ße, Charge: -1, Mass: N/A, Strength: Weak, Blocked by: metal/wood, Attracted to positive

Describe Gamma decay particle

Symbol: γ, Charge: N/A, Mass: N/A, Strength: very strong, Blocked by: 18" thick Pb, Attracted To: N/A

What is Nuclear Fission?

A heavy nucleus splits into two lighter more stable nuclei.

What is Nuclear Fusion?

2 lighter nuclei come together to form one heavy more stable nucleus.

What is Half-life?

The time it takes for ½ of sample to decay.

Where are the s block elements located on the periodic table?

Groups 1 and 2 and He

Where are the p block elements located on the periodic table?

Groups 13-18

Where are the d block elements located on the periodic table?

Groups 3-12

Where are the f block elements located on the periodic table?

Bottom 2 'rows'

What are valence electrons?

Outermost electrons.

What is the periodic law?

Elements in the same group/family have similar physical properties.

Where are metals located on the periodic table?

Left of stairs (except H).

What are the properties of metals?

Malleable, ductile, conductor, high melting/boiling pt.

Where are non-metals located on the periodic table?

Right of stairs (and H).

What are the properties of non-metals?

Insulator, don't conduct, low melting and boiling points.

Where are metalloids located on the periodic table?

Touch stairs (not Al).

What are the metalloid elements?

B, Si, Ge, As, Se, Te.

What are the properties of metalloids?

Semiconductors.

Where are Alkali Metals located?

Group 1 (not H).

What is the charge of Alkali Metals?

1+

Where are Alkaline Earth Metals located?

Group 2.

What is the charge of Alkaline Earth Metals?

2+

Where are Transition Metals located?

Groups 3-12.

What are some properties of Transition Metals?

Form color ions, each charge is a different color.

Where are Halogens located?

Group 17.

What is the charge of Halogens?

1-

What are the properties of halogens?

Most reactive nonmetals.

Where are Noble Gases located?

Group 18.

What are the properties of Noble Gases?

Nonreactive, inert.

Define Atomic Radius.

Size of atom.

Define ionic radii

size of ion (atom w/charge)

what is metallic activity?

how easily the atom will lose e-

Define Ionization Energy.

Energy needed to lose an electron.

Define Electronegativity/Electron Affinity.

How easily the atom gains electrons.

Why do atoms bond?

To become stable, full outer energy level/shell, 8 valence electrons.

What do Metallic bonds involve?

Only metals, sea of electrons, delocalized electrons.

What do Ionic compounds involve?

Cations and anions, transfer of electrons, charged ions.

What do Covalent molecules involve?

Nonmetals, sharing of electrons.

What is the octet rule?

Atoms want 8 electrons to be stable. Except hydrogen who only needs 2 electrons.

What electronegativity difference is for Ionic bonds?

above 1.7

What electronegativity difference is for Polar Covalent bonds?

.3-1.7

What electronegativity difference is for Nonpolar Covalent bonds?

below .3

List three types of intermolecular forces.

London Dispersion, Dipole-Dipole, Hydrogen Bonding

Name examples for London Dispersion

CO2, diatomic (nonpolar)

Name examples for Dipole-Dipole

PH3

Name examples for hydrogen Bonding

HF, NH3, H2O

describe single bond.

shares 2 electrons, is long and weak

describe double bond.

shares 4 electrons, is middle length and middle strength

describe triple bond.

shares 6 electrons, is shortest and strongest

What elements are in ionic bonds?

cation and anion

What elements are in covalent bonds?

nonmetal and nonmetal

What elements are in transition metals ionic bonds?

group 3-12 and nonmetals

define metallic bonds conductive properties

malleable, ductile, conducts, luster, high melting/boil point

define ionic bonds conductive properties

brittle, hard, conducts when molten/dissolved high melting/boil point, soluble in H2O

define covalent molecule bonds conductive properties

soft, NEVER conducts, good insulator, low melt/boil point insoluble, rigid

How do you know if the molecule is polar?

asymmetrical and/or has lone pairs around center.

How do you know if the molecule is NONpolar?

symmetrical and/or has no lone pairs around center.

What are the chemical change indicators?

Forms a precipitate, change color, forms a gas, change in energy

what are the types of gases?

Oxygen, Hydrogen, Carbon Dioxide

How do you know you have produced Oxygen gas?

re-ignites a glowing splint(coffee stirrer).

How do you know you have produced Hydrogen gas?

pops in the presence of fire.

How do you know you have produced Carbon Dioxide gas?

puts out fire.

Exothermic versus Endothermic

test tube becomes hot versus test tube becomes cold

For a reaction with a test tube becoming hot what side of the equation is on and what sign is AH?

lose/release energy, product side(right), negative

For a reaction with a test tube becoming COLD what side of the equation is on and what signed is AH?

gain/absorb energy, reactant side (left), positive

Acid/Base neutralization

double replacement type of reaction

Combustion reactions involve and to produce and _

hydrocarbon and oxygen produce CO2 and H2O

What are the steps of the chemical equation?

Convert to mol, Use mol ratio(Coefficient), Convert to unknown Unit

What is the empirical formula?

reduced form

What is the molecular formula?

not reduced

What is this formula for: % Composition by mass?

Part/Whole x100

Kinetics…Collision Theory requirements

Particles must collide, Particles must have enough energy, Particles must collide at the correct orientation

Reaction rate is proportional to the number of collisions

effective

increase surface area: more/increase/same number collision/rate

increase number collisions increase rate

define catalyst

increases the rate of rxn by allowing an alternative pathway with lower Ea

Equilibrium expression

products over reactants raised to their coefficients, solids and liquids are not included.

Properties of Acid

Reacts with certain metals,Has a pH of 2, Can turn litmus paper pink, Tastes sour., Can turn litmus paper pink., Keeps p clear(when added to base), High Amount of Hydrogen Ions than Hydroxide Ions

Properties of Base

Has a pH of 8, Can turn litmus paper blue, Tastes bitter.,Feels slippery,Contains more hydroxide ions than hydrogen ions,Turns phenolphthalein pink.,Doesn't react with certain metals.

Properties of Neutral

Has a pH of 7,Occurs when a strong acid reacts with a strong base,Contains equal hydroxide ions and hydrogen ions.

Strong Acid/Base versus Weak Acid/Base

Strong Acid/Base ionizes completely versus Weak Acid/Base ionizes partially

define concentration

n=CV, C=concentration and V=volume

What is the formula for dilution?

C1V1=C2V2

definition of Solutions

homogeneous mixtures, because can't see solute seperatly from solvent

solution, element or compound

magnesium sulfate-cmpd, air-solution, water-cmpd, brass-solution, element-copper solution-salt water

definition electrolyte

cmpd that breaks into ions and will conduct electricity

solute

the dissolving substance

solvent

the dissolving medium

Electrolyte

conduct electricity

def Solution Equilibrium: Unsaturated

less than max dissolve dot under the line

Solubility of gases: temperature/ pressure on gasses

increase pressure the gas solubility increase but decrease temperature the gas solubility