Aleks Placement Test: Chemistry

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Ethane

2 carbon

molecular compound

2 or more DIFFERENT atoms -covalently bonded

molecular element

2 or more atoms of the SAME element

Pentane

5 carbon

Wave-Particle Duality of Light

Light sometimes acts like a particle and sometimes like a wave

Dilution

M1V1 = M2V2

Ionic Bonds

Metal looses the electron and nonmetal gains it; the farther apart they are on the table the more likely it's ionic

Electromagnetic Spectrum

The range of wavelengths or frequencies over which electromagnetic radiation extend

Molecule

The smallest particle that has any of the properties of a compound

Plasma

The state of matter with the highest energy; it uses ionization instead of bonds

Bose-Einstein Condensate

The state of matter with the lowest energy; basically a very cold solid

Half-Life

The time required for half of the original sample of nuclei to decay; each radioactive nucleus of the same element has the same half-life; the shorter the half-life, the more likely a nucleus will decay

Combination Reaction

Two or more compounds form to make one compound.

Mixture

Two or more substances that are together but not bonded

Precipitation Reaction

Two solutions of soluble salts are mixed, resulting in an insoluble solid (precipitate) forming.

Atoms and Colors

When an atom is excited by energy it gives off its own characteristic colors of light

Visible Light

White light is passed through a prism and creates all visible colors; each color has its own frequency and wavelength

Zinc

Zn(2+)

Hypo (Cl & Br & I) ite

__O (-)

(Cl & Br & I) ite

__O2 (-)

(Cl & Br & I) ate

__O3 (-)

Per (Cl & Br & I) ate

__O4 (-)

_______ite

_______ous acid

______ate

______ic acid

Hydrogen Bond

a weak bond between two molecules resulting from an electrostatic attraction between a proton in one molecule and an electronegative atom in the other (N, O, F)

Bright Line Spectrum

a.k.a. emission spectrum; occurs due to the energy an electron gives off as it travels from high to low energy; fireworks

Ionic Bond

between metal and nonmetal

Covalent Bond

between two nonmetals

charge: 0 mass :1

charge and mass of a neutron

charge: +1 mass: 1

charge and mass of a proton

charge: -1 mass: 0

charge and mass of electron

mixture

contains many different components

pure substance

contains only one component has characteristic properties

g atoms given x 1 mol/mass of element finding

conversion to find moles

no

does the composition of a compound ever change?

Activation Energy Graph

download from reactants to loop other is either energy absorbed or released

condensation

gas --> liquid =

deposition

gas --> solid

vertical rows

groups

7

hepta

degree kelvin given - 273

how to find celsius

273 + degree of celsius given

how to find kelvin

dipole points toward more electronegative

how to tell electronegativity?

evaporation

liquid --> gas =

freezing

liquid --> solid

What happens with catalyst? <catalyzed reaction>

lowering of activation energy

groups with letter A

main group elements have letter ____

weight of moles x weight of element/1 mole

mole to mass conversion

protons, neutrons

more ______ you have, more _____ you need

positive

move decimal to left, positive or negative?

negative

move decimal to right, positive or negative?

atomic number

number of protons =

dipole dipole

occur between polar molecules

5

penta

horizontal rows

periods

octet rule

predicts preferred bonding patterns for many main group non metals

Gay Lussac Law

pressure and temperature P1/T1 = P2/T2

Boyle's Law

pressure and volume P1V1 = P2V2

Polymerization

process of reacting monomer molecules together in a chemical reaction to form polymer chains or three-dimensional networks.

lewis dot symbol

shows the valence e- for an element

sublimation

solid --> vapor

hydrogen, dipole dipole, dispersion

strongest to weakest forces

4

tetra

henrys law

the solubility of a gas in a liquid is proportional to the pressure of the gas above that liquid

mass number

total number of proton and neutrons in the nucleus =

Methane

1 carbon

Propane

3 carbon

Speed of Light

3.00•10^8m/s

Butane

4 carbon

Speed

How fast a wave travels in a given distance

Atomic Radius

The radius of an atom; decreases as you move left to right and increases as you move top to bottom

Covalent Bonds

Atoms are sharing electrons; the closer the elements are the more likely it's covalent

Borate

BO3(3-)

Polar Covalent Bonding

Bond where electrons are shared unequally

Bromate

BrO3(-)

Acetate

C2H3O2(-)

Oxalate

C2O4(2-)

Cyanide

CN(-)

Carbonate ?

CO3(2-) insoluble

Cadmium

Cd(2+)

Cobalt

Co(2+) & Co(3+)

Dichromate

Cr2O7(2-)

Chromate

CrO4(2-)

Copper

Cu(+) & Cu (2+)

Combustion Reaction

CxHy + O2 -> CO2 + H2O

IMF Scale

Dipersion < Dipoles < Hydrogen

Compound

Elements combine to form chemical compounds

Celcius & Fahrenheit

F=1.8C+32

Iron

Fe(2+) & Fe (3+)

Molar Mass

Found by summing the masses of the component atoms

Strong Acid (6)

HCl HBr HI HNO3 H2SO4 HClO4

Neutralization Reaction

Acid + Base -> Salt + H2O

Organic Acid

Acid that contains a carbon atom

Diprotic Acid

Acid that has 2 hydrogens to donate

Triprotic Acid

Acid that has 3 hydrogens to give

Oxyacid

Acid that has an oxygen

Silver

Ag(+)

Neutralisation Reaction

An acid and a base react with each other. Generally the product of this reaction is a salt and water.

Cation

An atom that looses electrons and has a positive charge; metals

Element

Any substance that contains only one kind of an atom

Matter

Anything that has mass and takes up space; made of atoms

Arsenite

AsO3(3-)

Arsenate

AsO4(3-)

Periodic Trends (1) Electronegativity (2) Ionization Energy (3) Electron Affinity (4) Atomic Radius

(1) & (2) & (3) increase towards top right (4) increase towards bottom left

polar

-electrons are not shared equally

nonpolar

-even electron distribution

dipole dipole forces

-stronger attraction -only polar molecules

dispersion forces

-weak attraction -non polar and polar molecules

Celcius & Kelvin

0 C = 273.15 K K= C+273.15

6.022 x 10^23

1 mole =

Hexane

6 carbon

Avogadro's number

6.022 X 10 ^ 23

(F-32) x 5/9

= celsius

c x 9/5 +32

= farenheit

polar

> 0.4 means it is

Polar Covalent Bond

A bond between 2 nonmetal atoms that have different electronegativities and therefore have unequal sharing of the bonding electron pair.

Nonpolar Covalent Bond

A bond between 2 nonmetal atoms that have the same electronegativity and therefore have equal sharing of the bonding electron pair.

Decomposition Reaction

A complex molecule breaks down to make a simpler one.

Base

A substance that decreases the hydrogen ion concentration in a solution.

Acid

A substance that increases the hydrogen ion concentration of a solution.

Ionic Compound

Metals often react with nonmetals to form ionic compounds. These compounds are composed of positive and negative ions formed by adding or subtracting electrons from neutral atoms and molecules.

Manganese

Mn(2+) & Mn(3+)

Permanganate

MnO4(-)

Ammonium

NH4(+) compounds are soluble

Nitrite

NO2(-)

Nitrate ?

NO3(-) compounds are soluble

Covalent Compound

Nonmetals combine with each other to form covalent compounds, which exist as neutral molecules.

Peroxide

O2(2-)

Cyanate

OCN(-)

Hydroxide ?

OH(-) insoluble

Hydrogen Bonding

Occurs between hydrogen and F, N, or O

Displacement Reaction

One element trades places with another element in the compound.

Combustion Reaction

Oxygen combines with a compound to form carbon dioxide and water. These reactions are exothermic, meaning they give off heat.

Phosphite

PO3(3-)

Phosphate

PO4(3-)

Ideal Gas Law

PV = nRT R: 0.08206 L atm / mol K 8.314 J / mol K

Lead

Pb(2+) & Pb(4+)

PH Scale

Ranges from 1 to 14, with 7 considered to be neutral. *pH less than 7 is said to be acidic *pH greater than 7 are basic or alkaline.

Lewis Structures

Represent the valence electrons

Thiosulfate

S2O3(2-)

Thiocynate

SCN(-)

Sulfite

SO3(2-)

Sulfate ?

SO4(2-) most are soluble -> except Ba Hg Pb

Tin

Sn(2+) & Sn(4+)

Five states of Matter

Solids, liquids, gases, plasmas, and Bose-Einstein condensates

Pure Substance

Substance that contains only one kind of compound

Avogadro's Law

volume and number of moles V1 / n1 = V2 / n2

Charles Law

volume and temperature V1/T1 = V2/T2

exchange of gases between the lungs and the blood

what does henrys law explain?

london dispersion

what force exists between ALL particles?

F, O, N

what must hydrogen be bonded to to be considered hydrogen bonding?

Neutron Number

Atomic Mass - Atomic Number

Characteristics of Metals

- Malleable - Ductile - Conductive - Lustrous

Decane

10 carbon

Planck's Constant

6.626•10^-34 Joules/hertz

Heptane

7 carbon

Octane

8 carbon

Nonatne

9 carbon

Photon

A light particle

Wave-Mechanical Model of the Atom

A model of the atom in which the orbitals are nothing like orbits

Plum Pudding Model

A model of the atom that depicts a sphere of positive charge with electrons scattered throughout

Radioactive

A nucleus that spontaneously decomposes, forming a different nucleus and producing one or more particles; alpha, beta, and gamma ray

Atomic Mass

A number that tells the number of protons and neutrons in an atom

Elements

A pure substance that contains only one type of atom

Atomic Orbital

A region around the nucleus of an atom where an electron with a given energy may be found 90% of the time; 4 types: s, p, d, and f

Pauli Exclusion Principle

A rule that states that each electron has its own unique set of quantum numbers and that two electrons with the same spin cannot occupy the same orbital and that an orbital can only hold two electrons

Gas

A state of matter with no bonds

Solid

A state of matter with strong bonds

Liquid

A state of matter with weak bonds

Atomic Number

A unique number to each element that tells the number of protons and the number of electrons if the atom is neutral

Acids

Always start with hydrogen; donate a proton in a solution

Anion

An atom that gains electrons and has a negative charge; nonmetals

Isotope

An atom that has changed its number of neutrons

Ion

An atom that has gained or lost electrons

Law of Constant Composition

Atoms of one element can combine with other elements to form compounds; a given compound always has the same relative numbers and types of atoms

Percent Abundance Equation

Average Mass = (%)•(Mass of Isotope A) + (%)•(Mass of Isotope B) +...

Atoms

Basic unit of matter which cannot be broken down and contain mostly empty space; contains three parts: the electron, proton, and neutron

Continuous Spectrum

Broken bands of colored light

Speed of Light Equation

C = w•f C is the speed of light w is wavelength in meters f is frequency in hertz

Ernest Rutherford

Conducted an experiment in which he shot alpha particles at gold foil; roved there was a small, dense nucleus with a positive charge and that protons are positive

J.J. Thomson

Discovered electrons and protons and developed the plum pudding model of an atom

Energy using Planck's Constant

E = h•f E is energy h is Planck's constant f is frequency in hertz

Hund's Rule

Each suborbital will fill with one electron before accepting a second electron

Kernel Structure

Electron configuration shorthand 1. Find the noble gas that comes before the element 2. Write the gas in brackets 3. Determine energy level and orbital you are starting on 4. Follow the energy pyramid

Valence Electrons

Electrons on outer most orbital; always the highest energy 's' and 'p' orbital

Percent Abundance

Elements exist naturally in different isotopes, to the atomic mass listed on the table is an average

Metals

Elements located on the left side of the periodic table that want to lose electrons

Nonmetals

Elements located on the right side of the periodic table that want to gain electrons

Metalloids

Elements placed in a stair-step line between metals and nonmetals; they have characteristics of both

Diatomic Molecules

Elements that occur in pairs in their natural state; hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

Robert Boyle

First to define an element; any substance is a substance unless it can be broken down

Heisenberg Uncertainty Principle

It is impossible to know the exact position and momentum of an electron at the same time

Alpha Particle

One type of radioactive particle; it is a essentially a helium nucleus; when this type of particle is released, the mass of the atom is conserved and so is the atomic number

Gamma Ray

One type of radioactive particle; it is a high energy photon of light and is used to release excess energy; the atom is not changed at all

Beta Particle

One type of radioactive particle; it is essentially an electron; when this type of particle is released, the atomic mass is conserved and the atomic number gains one (a neutron is changed to a proton)

Node

Point on a wave where the wave returns to the zero line; a crest or trough is trapped between the two points

S

Quantum number that tells how an electron spins in an orbital

M

Quantum number that tells us the orientation of the orbital in space

Alcohols

Subtract a hydrogen and add a -OH group; add ol to end of name

Electronegativity

The ability of a molecule to attract electrons to it; increases as you move left to right in the table and decreases as you move top to bottom; fluorine is the hardest

Conductive

The ability to allow heat or electricity to pass through an object

Malleable

The ability to be molded into shapes

Ductile

The ability to be pulled into wire

Lustrous

The ability to be shiny

Wavelength

The distance between the crests of a wave; symbol is lambda

Oxidation State

The electrons an element will gain or lose in order to become stable (8 electrons)

Ionization Energy

The energy needed to rip off an electron; increases as you move left to right and decreases as you move top to bottom

Amplitude

The height of a crest or trough; crest to the zero line; absolute value

Crest

The highest point of a wave

Trough

The lowest point of a wave

Electrons

The negatively charged particle in an atom; circles around the nucleus in the electron cloud

Neutron

The neutral particle in an atom; it has no charge and is located in the nucleus

Frequency

The number of waves that pass through a point in a given time; symbol is nu

L

The orbital quantum number; tells us the shape of the orbital (s,p,d,f)

F Orbital

The orbital with the highest energy; it has seven orbitals and can hold 14 electrons

S Orbital

The orbital with the lowest energy; it has one orbital and can hold two electrons

D Orbital

The orbital with the second highest energy; it has five orbitals and can hold ten electrons

P Orbital

The orbital with the second lowest energy; it has three orbitals and can hold six electrons

Proton

The positively charged particle in an atom; located in the nucleus; determine the element

N

The principal quantum number; tells us which energy level an electron is found in, the maximum number of electrons that can be found in one energy level, and the size of an electron cloud

Quantum Theory for an Atom

The probability of finding electrons in certain regions of an atom is described by orbitals

Compound

Two or more elements that are chemically bonded; includes ionic and covalent

John Dalton

Used and combined previous ideas to discuss the atom; elements are made of atoms; all atoms of an element are identical; atoms of different elements are different; law of constant composition; atoms are invisible

Dark Line Spectrum

a.k.a. absorption spectrum; occurs due to the energy that an electron gains as it travels from low to high energy


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