General Chemistry 1: Exam 1

Majority of the things are conceptual and not the actual math equations Also, for the SI conversions, I the exponents appear as subscripts for some reason, but they’re not. The numbers should be exponents.

tera (T)

1×10¹²

giga (G)

1×10⁹

mega (M)

1×10⁶

kilo (k)

1×10³

hecto (h)

1×10²

deka (da)

1×10¹

deci (d)

1×10^-1

centi [c]

1×10^-2

milli (m)

1×10^-3

micro (µ)

1×10^-6

nano (n)

1×10^-9

pico (p)

1×10^-12

femto (f)

1×10^-15

ºCelcius to Kelvin

K = ºC + 273.15

Kelvin to ºCelcius

ºC = K - 273.15

ºCelcius to ºFarenheit

ºF = (ºC × 9/5) + 32

ºFarenheit to ºCelcius

ºC = (ºF - 32) × 5/9

Atomic symbol, number, and mass

X = Atomic symbol of the element

A = mass number; A = Z + N

Z = atomic number (number of protons in nucleus)

N = number of neutrons in nucleus

Periodic Table Information

Rows = periods (electron shells)

Columns = Groups (valence electrons present)

Yellow = Akali Metals

Orange = Akali Earth Metals

Blue = Transition Metals

Navy = Post Transition Metals

Gray = Metalloids

Pink = Nonmetals

Light Blue = Halogens

Purple = Noble Gasses

Lewis Structure Example

Two dots = lone pair

One dot = covalent bonds possible

Periodic Table with Charges

Polyatomic ion

A charged species consisting of two or more atoms covalently bonded together

ammonium

NH₄ ⁺

nitrite

NO₂ ^-

nitrate

NO₃ ^-

sulfite

SO₃²

sulfate

SO₄^2-

hydrogen sulfate (aka: bisulfate)

HSO₄^-

thiosulfate

S₂O₃^2-

oxalate

C₂O₄^2-

hydroxide

OH^-

peroxide

O₂^2-

cyanide

CN^-

phosphite

PO₃^3-

phosphate

PO₄^3-

hydrogen phosphate

HPO₄^2-

dihydrogen phosphate

H₂PO₄^-

perchlorate

ClO₄^-

chlorate

ClO₃^-

chlorite

ClO₂^-

hypochlorite

ClO^-

bromate

BrO₃^-

iodate

IO₃^-

acetate

CH₃COO^-

and/or

C₂H₃O₂^-

carbonate

CO₃^2-

hydrogen carbonate (aka: bicarbonate)

HCO₃^-

chromate

CrO₄^2-

dichromate

Cr₂O₇^2-

permanganate

MnO₄^-

cyanate

OCN^-

thiocyanate

SCN^-

Naming binary compounds

Prefixes and name endings for compounds

Common names of compounds

Avogadro’s number:

1 mol = 6.022×10²³

Calculating % composition

% of element = (mass of specific element/mass of whole compound) x100

Calculating % yield

% yield = (actual yield/theoretical yield) x100

significance of the photoelectric effect experiments on understanding of atomic structure (part 1)

- Electrons ejected when frequency over a threshold frequency

- Size of current is proportional to the intensity of incident light

significance of the photoelectric effect experiments on understanding of atomic structure (part 2)

• Electrons ejected when frequency over a threshold frequency

• Size of current is proportional to the intensity of incident light

Describe the electronic structure of the atom in terms of energy levels

Closer to nucleus = lower E

• e^- prefer to occupy lowest E state available

In the ground state of the atom

• all e^- are in lowest possible E level

How do electrons move between energy levels within the atom

To move to a higher E level

• the e must absorb a photon

• that has the correct v and E

• E must match ΔE between levels.

To drop back to a lower E level

• the e must emit a photon

• with the correct v and E.

What is C?

• speed of light

• 2.998×10⁸ m/s (constant)

• c = ⋎*λ

What is ⋎?

frequency

• ⋎ = c/λ

What is λ?

Wavelength

• λ = c/⋎

What is h?

6.626 × 10^-34 J*s (constant)

How do you find E?

E = (h x c)/(λ)

( 6.626 × 10^-34J*s x 2.998 × 10⁸m/s )/(λ)