midterm general chem I

nitrite

NO₂⁻

nitrate

NO₃⁻

sulfate

SO₄²⁻

sulfite

SO₃²⁻

hydrogen sulfate

HSO₄⁻

hydrogen sulfite

HSO₃⁻

thiosulfate

S₂O₃²⁻

perchlorate

ClO₄⁻

chlorate

ClO₃⁻

chlorite

ClO₂⁻

hypochlorite

ClO⁻

phosphate

PO₄³⁻

hydrogen phosphate

HPO₄²⁻

dihydrogen phosphate

H₂PO₄⁻

azide

N₃⁻

acetate

C₂H₃O₂⁻

ammonium

NH₄⁺

hydronium

H₃O⁺

cyanide

CN⁻

hydroxide

OH⁻

peroxide

O₂²⁻

chromate

CrO₄²⁻

dichromate

Cr₂O₇²⁻

permanganate

MnO₄⁻

carbonate

CO₃²⁻

bicarbonate

HCO₃⁻

hydronium

H₃O⁺

mono

1

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

10

deca

whats in box 1

alkali metals

whats in box 2

alkali earth metals

whats in box 3

metals

whats in box 4

transition metals

whats in box 5

lanthanides

whats in box 6

actinides

whats in box 7

noble gases

whats in box 8

halogens

whats in box 9

non metals

whats in box 10

metalloids

whats the charge of the highlighted elements

+1

whats the charge of the highlighted elements

+2

whats the charge of the highlighted elements

+1

whats the charge of the highlighted elements

+2

whats the charge of the highlighted elements

+3

whats the charge of the highlighted elements

-2

whats the charge of the highlighted elements

-1

what is the charge of aluminuum

3+

charge of cadmium(Cd) and zinc (Zn)

2+

Charge of Ag?

+1

what does the staircase represent

metalloids

what did John dalton do

proposed atomic theory suggesting matter is made of atoms

law of definite and proportions

all samples of a pure compound contain same elements in same proportions by mass

law of multiple proportions

2 elements can form more than 1 compound

jj thompson

discovered electrons thru cathode ray finding that the ray deflected towards positive poles making the ray negatively charged

Robert a Millikan

used oil drop experiment to advance electrons showing the charges of electrons

Ernest rutherford

discovered most alpha particles passed thru gold foil but some deflected

What is matter

Anything that takes up space and has mass

Physical vs change

Physical change is just a rearrangement of what you already have while chemical causes something new to form

What do pure substances consist of

Elements and compounds

Explain particles

Atoms that attract each other and are constantly floating

Intensive vs extensive

Extensive depends on how much you have while intensive does not

What are mixtures composed of

Hetero and homogenous mixtures

What’s differentiating

Finding the odd one out

Rules of sig fig

#’s 1-9

Zeros between #’s count (808)

Trailing zeros count if theres a decimal (200.0)

Zeros at the beginning before a # dont (0.0034)

Finding accuracy

How close a measurement is to the true value

Finding precision

How close a series of measurement are to each other

Conversion for kelvin temp

C + 273.15

Compound

Two diff elements together

Molecules

Two of the same element together ( N2)

Symbol and conversion of kilo

X10³ k

Symbol and conversion for nano

X10^-9 n

Symbol and conversion of mili

X10^-3. m

Symbol and conversion for micro

X10^-6. μ

Symbol and conversion for centi

X10^-2. c

Density formula

D= mass/volume

Volume formula

Volume= LxWxH

If you’re a pure substance what type of mixture are you

Homogenous

Ionic compounds

Meta and nonmetal

Molecular compounds

Nonmetal and nonmetal

How do you find formula mass

By using the atomic mass and adding them up

Diff between binary and oxoacid

Binary has NO OXYGEN

Steps to naming a molecular formula

Steps to naming a ionic compound

Naming oxoacid steps

Naming binary acids

Cations

Positive ions that lose an e-

Anions

Negative ions that gain e-

Ground state

The lowest energy electronic configuration possible for an atom.

Excited state

Any electronic state of an atom that has higher energy than its lowest possible energy state.

Relationship between wavelength and energy

Inversely proportional; as wavelength decreases, photon energy increases.

Principal quantum number ($n$)

how far an e- is from nucleus

where $n$ is a positive integer ($1, 2, 3, \dots$).

Secondary quantum number ($l$) or azimuthal

energy and shape of the orbital,

integer values ranging from $0$ to $n - 1$.