ACS GEN CHEM 1 FINAL

the physical material of the universe. It is anything that has mass and occupies space.

Matter

is made up of relatively few elements.

Matter

The smallest building block of matter. Smallest particle that retains the chemical property of the element (O, He, S).

Atom

Each _______ is made of the same kind of atom

Element

Combination of atoms held together in specific shapes

Molecule

No fixed volume or shape, conforms to

volume and shape of container, is compressible

Gas

Individual particles are confined to a given volume, liquid flows (no definite shape) and assumes the shape of its container up to the volume of the liquid, slightly compressible

Liquid

Rigid with definite shape, very slightly compressible

Solid

these stable diatomics

H2,O2, N2, and the Halogens (F2, Cl2, Br2, I2)

Different samples of any pure compound contain the same elements in the same proportion by mass

Law of Constant (Definite) Composition

characteristics of a substance. Can be observed without changing a substance into another substance

Physical Properties

Describes the reactivity of a substance. Can only be observed when a substance is changed into another substance

Chemical properties:

Does not depend on amount.

Intensive property :

Depends on amount.

Extensive property

Substances transform into chemically different substances

Chemical change

No change in chemical composition

Physical change

How close to the true value a given measurement is.

Accuracy

How well a number of independent measurements agree with one another.

Precision

Electrons were discovered by ______ in 1897, while

Millikan's Oil Drop experiment determined its charge.

• Neutrons were discovered by James Chadwick in 1932.

J.J. Thompson

Postulated a very small, dense nucleus with the electrons around the outside of the atom. Most of the volume of the atom is empty space.

Rutherford

Protons were discovered by______in 1919.

Rutherford

Neutrons were discovered by________ in 1932.

James Chadwick

1) All matter is made of atoms. Atoms are indivisible and indestructible.

2) All atoms of a given element are identical in mass and properties

3) Compounds are formed by a combination of two or more different kinds of atoms.

4) A chemical reaction is a rearrangement of atoms.

Dalton's Atomic Theory

Organic alkANEs

Mother Eats Peanut Butter:

Methane: CH4

Ethane: C2H6

Propane: C3H8

Butane: C4H10

...then greek prefixes

Uniform throughout, air, milk, sea water

Homogeneous mixture

Not uniform, chocolate chip cookie

Heterogenous mixture

When an element has a change in mass number, or neutrons

isotope

A species of an element in which the number of electrons does not equal the number of protons.

Ion

Each isotope of an atom has a different number of neutrons.

Isotope

mols/L; mmols/mL

Molarity

The lighter a gas's atomic weight, the faster it will escape a container.

Graham's Law of Effusion

The temperature at which the solid and liquid phases of a substance are in equilibrium at atmospheric pressure (760 mm Hg).

Normal Melting Point

The point at which the vapor pressure of a liquid equals 1 atm.

Boiling Point

change in spontaneity of a system.

Free Energy

Amount of energy required to raise the water surrounding the chamber of the bomb calorimeter by one °C

Calorimeter Constant

ΔG = ΔH - TΔS, where ΔH = change in enthalpy and ΔS = change in entropy.

Gibbs Free Energy

change in energy of a system.

Enthalpy

change in chaos of a system.

Entropy

Two atoms with the same charge.

Isoelectric

An insulated container used to study reactions at a constant volume.

Bomb Calorimeter

Same as specific heat, but requirement for raising 1 mole of a substance by one °C.

Molar Heat Capacity

The energy required to break a bond, and the energy released when a bond is formed.

Bond Energy

The component of a chemical reaction that will be completely used up first.

Limiting Reagent

Can be g/mol, kg/kmol, mg/mmol, etc.

Atomic Mass

The amount of heat required to raise the temperature of one gram of a substance by one °C. (units: J x g⁻¹ x °C⁻¹)

Specific Heat

(J) mass (g) x specific heat (J x g⁻¹ x °C⁻¹) x ΔT (°C)

Heat (q)

A covalent bond in which the two electrons derive from the same atom; occurs most often between Lewis acids and bases.

Coordinate Covalent Bonding

22.414 L/mol @ STP

Molar Volume of an Ideal Gas

The volume occupied by one mole of a substance.

Molar Volume (Vm)

CxHy + (x + y/4)O₂ → xCO₂ + y/2H₂O

Combustion of a Hydrocarbon

Two molecules that are composed of the same type and number of elements but are arranged in different ways and have different properties are isomers.

Isomer

V - N - (B/2) where V = total valence e⁻, N = non-bonding e⁻, and B = bonding e⁻.

Formal charge

Has a unique structure; O-Si-O bonds are always 109.5°.

Silicon Dioxide

Mathematical procedure in which the standard atomic orbitals combine to form new orbitals.

Hybridization

Occurs when three atoms and one non-bonding pair is arranged around a central atom. Polar.

Trigonal Pyramidal

Arrangement of four objects around a central atom. Non-polar.

Tetrahedral

Occurs when one non-bonding pairs and two atoms are arranged around a central atom. Polar.

Bent

Arrangement of two objects around a central atom. Non-polar.

Linear

Orbital Composed of one s and one p orbital; can hold four electrons. Linear.

sp

Bonding occurs between orbitals that are side-by-side.

Pi Bonding

Orbital Composed of one s orbital and two p orbitals; can hold six total electrons. Trigonal planar.

sp²

Two atoms with the same number of neutrons.

Isotopic

Formed by head-on overlapping between orbitals.

Sigma Bonding

When hydrogen is attracted to electronegative atoms.

Hydrogen Bonding

Occur in the third row of the periodic table and beyond in elements that can form stable bonds with more than eight electrons. Eg. XeF₂

Expanded Octets

Occur in elements that can form stable bonds with less than eight electrons. Eg. BF₃

Incomplete Octets

The 4s orbital is filled before the 3d orbital, but listed after.

Transition Metal Orbitals

Compounds with an odd number of electrons in their Lewis Structure. Eg. NO₂

Free Radicals

The way that three objects will arrange themselves around a central atom. Non-polar.

Trigonal Planar

Orbital An orbital composed of one s orbital and three p orbitals; can hold eight total electrons. Tetrahedral.

sp³

A molecule that is mostly positive on one side and mostly negative on the other.

Polar Molecule

Two equally correct arrangements of one molecule's electrons; generally the molecule exists as an average of the two.

Resonance Structures

Tetrahedral Bond Angle

109.5°

to lose electrons and form positive ions.

Electropositive

Atoms that possess a permanent magnetic charge due to the presence of unpaired electrons.

Paramagnetic

only group to have all three phases

Halogens

also know as atomic weight

Average atomic mass

Metal atom + metal atom -->,"sea of electrons"

Metalic bonding

Non-metal atom + non-metal atom

covalent bonding

sharing of electrons

covalent bonding

metal atom + non-metal atom -->

ionic bonding

transferring of electrons

ionic

assemblies of two or more atoms bonded together

molecules

ethyl alcohol

C2H6O

give the actual numbers and types of atoms in a molecules

molecular formula

give the relative numbers and types of atoms in a molecule

empirical formula

metals usually form

cations

non-metals usually form

anions

the charge on one ion will become the ___ on the other

subscript

cations formed from metal will have

the same name as the metal

added to represent the lower charged cations

ous

added to represent the higher charged cations

ic

added to cations formed from non-metals

ium

added to the end of a monatomic anion (has 3 exceptions:)

ide

more than one atom but still +ide:

hydroxide, cyanide, peroxide

hydroxide

OH-

cyanide

CN-

peroxide

O2^2-

is added to the most common or sole oxyanion of the element

ate

ex. CO3^2- = carbonate, CrO4^2- = chromate

is used for an oxyanion with the same charge but one less O atom

ite

ex. SO4^2- = sulfATE but SO3^2- = sulfITE

NO3- = nitrATE, but NO2- = nitrITE

oxyanions with more than two members in the series are named:

(Halogens, except F)

per....-ate

-ate

-ite

hypo....-ite