Learn: Chem 102 (week 1-3)

What is science

the systematic study of the physical and natural world. involves observation and experimentation

3 measurements for a scientific fact

must be testable, repeatable, and reproducible

what 2 criteria must there be for applying duobt

questions must be testable and unbiased

define theory, hypothesis, and law

Hyp: an unproven idea, usually based on a set of observations. Law: an equation or statement that predicts an outcome without understanding how the result occurs. Theory: deep understanding of the mechanism of how a process occurs, make good predictions and gives insight on the process occurs

Solve for T1: V1/T1 = V2/T2

T1= T2xV1/V2

Solve for V2: V1/T1 = V2/T2

V2= V1xT2/T1

Rules of scientific notation

only has one number to the left of the decimal point (1-9), also only includes significant figures

Tera (T)

10^12

Giga (G)

10^9

Mega (M)

10^6

Kilo (K)

10^3

Deci (d)

10^-1

Centi (c)

10^-2

Milli (m)

10^-3

Micro (u)

10^-6

Nano (n)

10^-9

Pico (p)

10^-12

Femto (f)

10^-15

If one mile = 1.609km, how many miles are in 1 km?

*divide 1 mile by 1.609km

If 1 meter is 1.0936yards, how many meters are in a yard

*divide 1 meter by 1.0936 yards

Define accuracy and precision

Accu: refers to how close the measure value is to actual. Preci: refers to how close a series of measurements are to one another/how reproducible they are

Define exact and inexact numbers

Exact: values known with complete certainty. Inexact: come from things we measure and have uncertainty

Rules of significant figures

All non zero digits are significant

How many significant figures: 0.052

2

How many significant figures: 91

2

How many significant figures: 21.2

3

How many significant figures: 101

3

How many significant figures: 1.200

4

How many significant figures: 9600

2

How many significant figures: 960.0

4

How many significant figures: 0.17

2

How many significant figures: 99.80%

4

How many significant figures: 1.4 x 10^4

2

How many significant figures: 0.080

2

How many significant figures: 5.5000

5

What is chemistry

study of matter, at its most microscopic level

Definitions of an atom and element

- matter is the things that make up the universe, measurable and tangible

- an element is a substance made up of atoms, which has properties of an atom, it cannot be broken down into 2+ substances

- atoms are microscopic things, we can't see it or manipulate it directly

What is a proton (Charge, mass, and significance)

- the number of protons in the nucleus determines which element the atom is

- the atomic number of an atom is the number of protons in the nucleus

- every proton in the universe is the same, one positive unit of charge, and a mass of 1.6726x10^-27

What is a neutron (Charge, mass, and significance)

- the number of neutrons in the nucleus determines the mass/atomic weight

- every neutron is the same, has 0 charge and a mass of 1.6726x10^-27

What is an electron (Charge, mass, and significance)

- the number of electrons matches the number of protons in the nucleus

- atoms and elements have a neutral charge

electrons carry one negative unit of charge, and have a mass of 9.1093x10^-31

Why are atoms and elements considered to be charge neutral

electrons bind to the atom based on the number of protons, cancelling out the charge of each

Define isotopes

The same elements that have different masses

abundance equation

amu1(%-->0.hhh)) + amu2 (%-->0.hhh)

How do positive and negative charges on an atom effect number of electrons

+ = lose e-, - = gain e-

define ions

charged atoms due to an imbalance in #e- and #p+

Describe the electronic structure of atoms

locations of e- exist in energy series called orbitals, contain high energy

Energy series up to 3p

1s, 2s, 2p(3), 3s, 3p(3)

How many orbitals are in each energy series and how many electrons can they hold

1s, 2s, and 3s have 1 orbital each and can hold 2 e-. 2p and 3p have 3 orbitals each and can hold 6 e- total

energy series memorization

11 22 33 43 45, s p d f

Density equation

d = mass/volume

Mass and volume for density units

grams(g), milliliters (mL) or cubic centimeters (cm^3)

Density pyramid

M over D and V ;

M/D | V