General Chemistry ACS Study Guide

Isotopes

when the number of neutrons varies but it has the same number of protons ex) Ne-20 and Ne-22`

What was believed until the beginning of the 20th century?

That all physical phenomena were deterministic

Light

Form of electromagnetic radiation

What is electromagnetic radiation composed of?

perpendicular oscillating waves, one for the magnetic field and one for the electric field

Quantum number n

size, n>1

Quantum number l

shape, l=0 to (n-1)

Quantum number ml

orientation, -l to +l

s orbital

l=0, 1 orbital

p orbital

l=1, 3 orbitals

d orbital

l=2, 5 orbitals

f orbital

l=3, 7 orbitals

Electron configurations

description of the orbitals occupied by electrons

Valence electrons

in the electron configuration they are the electrons associated with highest principle valence shell orbital

Nonmetallic character trend

increases from left to right and bottom to top

Electron Affinity trend

get more negative from left to right and bottom to top

Ionization Energy trend

increases from left to right and bottom to top

Metallic Character trend

gets more metallic from right to left and top to bottom

Atomic Radius trend

increases from top to bottom and right to left

Naming molecular compounds

prefix+1st element+prefix+base name of 2nd -ide

Naming Ionic Compounds

metal w/ invariant charge=metal name

metal w/ variant charge= metal name(charge)

nonmetal= stem of name+-ide

Oxidation numbers

1-3. sum=charge

4. 1A=+1 2A=+2

5. F=-1

6.H=+1

7. O=-2

8. POLY

9. 7A=-1 6A=-2 5A=-3

How to draw Lewis Structure

1. determine valence e-

2. use bond calculator

3. draw Lewis Structure

2 electron groups, 0 lone pairs

Linear

3 electron groups, 0 lone pairs

Trigonal Planar

3 electron groups, 1 lone pair

Bent-120

4 electron groups, 0 lone pairs

Tetrahedral

4 electron groups, 1 lone pair

Trigonal Pyramidal

4 electron groups, 2 lone pairs

Bent 109.5

5 electron groups, 0 lone pairs

Trigonal Bipyramidal

5 electron groups, 1 lone pair

Seesaw

5 electron groups, 2 lone pairs

T-shaped

5 electron groups, 3 lone pairs

Linear

6 electron groups, 0 lone pairs

Octahedral

6 electron groups, 1 lone pair

square pyramidal

6 electron groups, 2 lone pairs

square planar

Kinetic Energy

energy that is being transferred

Potential Energy

energy that is stored in an object

Enthalpy(H)

the sum of internal energy of the system and the product of pressure and volume

Hess's Law

the change in enthalpy for a step wise process is the sum of the enthalpy changes of the steps

Standard Enthalpy of Formation

the enthalpy change for the reaction forming 1 ole of a pure compound from its constituent elements

Net ionic Equations

an ionic equation where all spectator ions are removed

stoichiometry

the study o the numerical relationship between chemical quantities in a chemical reaction

BCA table

efficient way to organize stoichiometric calculations

Molarity

moles of solute/ liters of solution

Dilution

the process of preparing a more dilute solution by adding solvent to a more concentrated solution

Matter

anything that occupies space and has mass

Pure substance

doesn't have variable composition

Mixture

has variable composition

Element

not separable into similar substances ex)Ne He Au

Compound

separable into similar substances ex) H2O

Heterogeneous

different throughout ex) wet sand

homogeneous

same throughout ex) tea with sugar

Physical Change

changes that alter the state or appearance of the matter without altering the composition ex) boiling water

Chemical Change

changes that alter the composition of the matter ex) rusting of an iron pole

Strong Acids

Hcl, HBr, HI, HNO3, H2SO4, HClO4

Strong Bases

1A and 2A hydroxides

Boyles Law

P1V1=P2V2, pressure is inversely related to volume

Charles Law

V1/T1=V2/T2, volume of gas is directly proportional to temperature

Avogadros Law

V1/n1=V2/n2 volume directly proportional to the number of moles

Combined Gas Law

P1V1/n1T1=P2V2/n2T2

Change from gas to solid

deposition

change from solid to gas

sublimation

change from solid to liquid

melting

change from liquid to solid

freezing

change from gas to liquid

condensation

change from liquid to gas

vaporization

Dispersion Force

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Hydrogen Bonding

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Dipole-Dipole Force

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