Chem Semester 1 Final

Different past experiences...

can result in different conclusions

Human...

pride/prejudice/beliefs

Too focused on one thing...

to notice other things

Focus v.

serendipity

Some things...

are just beyond our observation

Matter

anything with mass and volume

Pure matter

made up of only one kind of matter (elements and compounds)

Element

A pure substance made of only one kind of atom; cannot be broken down

Compound

A substance made up of atoms of two or more different elements joined by chemical bonds in fixed proportions

Mixture matter

two or more types of matter (homogeneous and heterogeneous)

Homogeneous matter

matter that has the same properties throughout the sample; transparent

Heterogeneous matter

a mixture consisting of physically different distinct substances; chunky

Solute

A substance that is dissolved in a solution.

Solvant

the substance in which the solute dissolves

Heat always flows from...

hot (loses heat, cools down) to cold (gain heat, heats up)

Extensive property

properties describing mass, shape, and dimensions of a particular peiece of matter

Intensive property

properties focusing on the substance (physical or chemical)

Physical properties

A characteristic of a pure substance that can be observed without changing it into another substance (color, density, ductility, malleability, melting/boiling points, conductivity, solubility, change in state)

Chemical property

A characteristic of a pure substance that describes its ability to change into different substances (decomposition, react w water, react w acids, burning, toxic, oxidation); usually heat is given off and new substance is formed

Solids

ridgid, fixed shape & volume, cannot be squashed

Liquids

not rigid, no fixed shape, fixed volume, cannot be squashed

Gases

not rigid, no fixed shapes or volume, can be squashed

Endothermic

a chemical reaction in which heat energy is absorbed

Exothermic

a chemical reaction in which heat energy is given off

Chemistry

the study of matter and how it changes

Ammonium

NH4+

Acetate

CH3COO-

Hydroxide

OH-

Nitrate

NO3-

Carbonate

CO3 2-

Sulfate

SO4 2-

Phosphate

PO4 3-

Ammonia

NH3

Nick the Camel ate Supper in Phoenix

vowels = charge

Photons

particles of light (wavelengths)

The shortest wavelengths are...

violet (gamma rays)

The longest wavelengths are...

red (radio waves)

White light is...

all the colors and colors can be seperated

Primary colors of light

green, blue, red (make white)

Ground state

when an atoms electrons are in the orbitals with the lowest energies

Excited state

when one or more electrons in an atom move from their ground state to orbitals with higher energies (comes back down and gives off a certain wavelength)

Quantum mechanics

describes the motions of subatomic particles and atoms as waves

Newtonian mechanics

The basic laws of motion, postulated by Newton, which are sufficient to explain and quantify virtually all of the complex dynamical behavior found on Earth and elsewhere in the universe.

Shape of s orbitals

sphere

Shape of p orbitals

peanut

Shape of d orbitals

four-leaf clover

Shape of f orbitals

odd combinations of shapes

Things that excite electrons

heat, light, electricity, chemical reactions, nuclear decay

Acronym for what excites electrons...

Harry Likes Eating Crunchy Noodles

Examples of heat electron excitement

flame lab, menthol demonstration, things that are "red hot", wood fire, fireworks

Lithium (Li) color in excited state

red

Sodium (Na) color in excited state

orange

Strontium (Sr) color in excited state

red

Copper (Cu) color in excited state

green

Potassium (K) color in excited state

purple

Examples of light electron excitement

fluorescence, fabric brighteners, black light, posters, phosphorescence, glowing bones and other glow things

Fluoresence

a photon creating a very brief excited state, 10^-9 to 10^-6 seconds, then when the electrons return to ground state a different type of photon is released

Phosphorescence

a photon creates a longer excited state, 10^-3 to several minutes

Examples of electricity electron excitement

lightnight, arc from an electrical shock, shock, fluorescent light bulbs, neon signs

Examples of chemical reaction electron excitement

glow sticks/necklaces, when anything is cracked and broken or shaken, bioluminescence

Bioluminescence

the production of light by means of a chemical reaction in an organism

Examples of nuclear decay electron excitement

radiation from atoms spewing protons and neutrons from nucleus, uranium glass, radioactive decay

Atomic spectra

the particular wavelengths (colors) an element emits

Maleable

the ability of metals to be beaten into sheets

Ductile

the ability to be drawn into a wire

Luster

the way a mineral reflects light from its surface (alkali metals)

Conductivity

the ability of an object to transfer heat or electricity to another object

Diatomic

molecule consisting of two atoms (nitrogen, oxygen, halogens)

Atomic radii trend

size of the atom; increases down and left

Electronegativity (electron affinity) trend

strength of attracting electrons; increases up and right

Density trend

mass per volume; increases up and towards the middle

Ionization energy trend

energy required to remove electrons; increases up and right

Allotropes

two or more different molecular forms of the same element in the same physical state

Alkalki metals produce \___ gas when placed in water

hydrogen

Lewis dot structures are only concerned with

s and p orbitals

Absorption spectra

a spectrum of electromagnetic radiation transmitted through a substance, showing dark lines or bands due to absorption of specific wavelengths.

Protons

positively charged particles in the nucleus (same size as neutrons)

Neutrons

neutrally charged particles in the nucleus (same size as protons)

Electrons

negatively charged particles outside the nucleus (MUCH smaller than protons and neutrons)

Ions

positively or negatively charged atoms created by a change in electrons

Mass number/atomic mass

number of protons plus the number of neutrons in an atom of an element

Atomic number

the number of protons in the nucleus of an atom

Hydrogen

H 1

Helium

He 2

Carbon

C 6

Nitrogen

N 7

Oxygen

O 8

Florine

F 9

Neon

Ne 10

Sodium

Na 11

Magnesium

Mg 12

Aluminum

Al 13

Silicon

Si 14

Phosphorus

P 15

Sulfur

S 16

Chlorine

Cl 17

Potassium

K 19

Calcium

Ca 20

Manganese

Mn 25

Iron

Fe 26