Introduction to Chemistry Concepts and Bonding

Organic chemistry

Study of most Carbon based compounds

Inorganic chemistry

Study of most non-organic substances (metals)

Physical chemistry

Study of the properties and changes of matter and their relation to energy

Annylitical chemistry

The identification of components and composition of materials

Biochemistry

The study of substances and processes occurring in living things

Theoretical chemistry

Use of math and computers to understand the principles behind observed chemical behavior and to design and predict properties of new compounds

Basic research

Used to expand knowledge

Applied research

Used to solve a problem

Technological development

The production and use of products to improve our quality of life

Matter

Anything with mass that takes up space

Atom

Smallest unit of matter that maintains the chemical identity of that element (ex. Hydrogen)

Element

A pure substance that cannot be broken down further and is made up of 1 type of Atom (ex. O2)

Compound

A substance that can be broken down and each compound is made of 2+ elements (ex. H2O)

Extensive properties

Dependent on the amount of matter (ex. Volume, mass, amount of energy) Like the time it takes a ice cube to melt

Intensive properties

Independent on the amount of matter (ex. Melting point/density)Things that will happen no matter the amount of density

states of matter

solid, liquid, gas, plasma

Solid

Definite volume and shape

Liquid

Definite volume and definite shape

Gas

No definite volume or shape

Plasma

High temperature state where atoms lose electrons

Physical properties

Can happen without changing its identity (ex. Melting point)

Chemical properties

A substance's ability to undergo change and when something transforms into something with a different identity (ex. firewood)

What is true in reactants and products?

Reactants always turn into products not the other way, energy is not created or destroyed, always involves energy

Mixture

A blend of 2+ kinds of matter where each retains its own identity and properties (ex. A bowl of apples and oranges)

Homogenous

Mixture with uniform composition (ex. Salt Water)

Heterogeneous

Mixture that is not uniform (ex. Different colors of skittles in the same bag)

Pure substance

Always heterogeneous / has a fixed composition

Groups/families

Vertical with similar properties

Periods

Horizontal with similarities

Metals

good conductors

non-metals

Bad conductors

Metalloids

Can be good or bad conductors

Silicone

semi-conductors

Types of data

Qualitative and quantitative

Qualitative data

Descriptive data that shows the quality of something

Quantitative data

Using numbers for data/shows the quantity of something

Hypothesis

Drawing conclusions from data to make a testable statement

Variables

Change between experiments

Controls

Do not change between experiments

Scientific method

Steps including observing, hypothesis, testing, theorizing, and publishing/results

Scientific Method: Observing

making an observation to gain information/ figure out what you want to test/prove

Scientific Method: Hypothesis

using that data to make an educated guess

Scientific Method: testing

test the hypothesis to see if it was true

Scientific Method: theorizing

review the test results

Scientific Method: publishing/results

share the result with others

Scientific theory

A theory that was made based on current data and can be used to explain something

Everyday theory

A theory that was not based on data and is more like a 'hunch'

what is the 'language used in sceinece?

SI units

SI units include...

Length, mass,time, amount of substance

length

represented as l, measured in meters, abbreviated as m

Mass

represented as m, measured in kilograms, abbreviated as kg

time

represented as t, measured in seconds, abbreviated as s

Amount of substance

represented as n, measured in mole, abbreviated as mol

Volume

cubic meter (m^3)

Density

Volume over mass (kg/m^3)

Equation for density

D=m/v

Giga

10^9 (1000000000) rep. as G

Mega

1,000,000 (10^6) rep. as M

Kilo

1,000 (10^3) rep. as k

Hecto

100 (10^2) rep. as h

Deka

10 (10^1) rep. as da

Deci

0.1 (10^-1) rep. as d

Centi

0.01 (10^-2) rep. as c

Milli

0.001 (10^-3) rep. as m

Micro

0.000001 (10^-6) rep. as µ

Nano

0.000000001 (10^-9) rep. as n

Accuracy

The closeness of a measurement to a known value.

Precision

The closeness of a set of data to each other.

Percentage error equation

Percent error = (Value experimental - Value accepted) / Value accepted × 100%

Significant figures rules

All nonzero digits are significant; zeros between nonzero digits are significant; leading zeros are not significant; trailing zeros after a decimal are significant; trailing zeros before a decimal are significant if there is a decimal point.

Multiplication and division rules for significant figures

The answer cannot have more significant figures than were used to obtain the answer.

Adding and subtracting rules for significant figures

Line up values and add/subtract, then adjust the answer to have the same number of decimal places as the number used with the least decimal places.

Scientific notation formula

m x 10^n, where m's value is between 1 and 10, and n is a whole number.

3 basic laws that describe chemical reactions

the conservation of mass, the law of multiple proportions, and the law of definate proportions

Conservation of mass

Mass will not be created or destroyed in chemical reactions.

Law of definite proportions

If different chemical compounds have the same two elements in the exact proportions by mass, they do not change based on sample size.

Law of multiple proportions

if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

What forms the beam in the cathode ray tube

Electrons

What happened to the beam when a positively charged magnet was brought towards it?

The beam went towards it

What happened to the beam when a negatively charged magnet was brought towards it?

the beam went away from it

How to find noble gas notation:

go up 1 row, to noble gases, write down, count how many to get back, fill in orbitals fro each chunk of periodic table and fill in the electrons

what did Earnest Rutherford do and find?

Preformed the gold foil experiment and found that the nucleus of the atom must be positively charged and dense

What do atoms have in their nucleus?

Protons and nuetrons

Atomic number

Tells us how many electrons and protons there are in an atom.

Isotopes

Atoms of the same element that have different masses.

Avogadro's number

6.033 x 10^23, which represents the number of atoms in one mole of a substance.

If you have the chart:

➡ ➡

Mass of element(g) Mass of element(mol) number of atoms in element(atoms)

⬅ ⬅

What do you do to fill in where the arrows are above and below?

Top: divide by molar mass (g/mol), multiply by avagadro's number

Bottom: multiply by the molar mass(g/mol), divide by avagadro's number

Wavelength

Measured in meters, called lambda (𝛌)

Plank's constant

Represented by (h), measured in (j/s)

Equation for Plank's constant

6.626x10^-3

Frequency

Number of waves that pass a specific point in a specific amount of time (seconds or s), units are (hz), represented as (v) and measured as (1/s)

Speed of light

Represented as (C), measured in meters per second (m/s), equation is 3.00 x 10^8

Equation for speed of light

𝛌 = c/v

Equation with speed of light, frequency and wavelength

C = 𝛌 * V (as frequenecy increases wavelength decreases

Energy

Represented as E, measured in joules