Matter (chemistry)

solid

- definite shape and volume -atoms are compressed -not easy to squeeze -orderly arrangement, highly organized, rigid, tightly packed particles -crystalline structure, lattice repeating pattern -dense (pressure has little effect) -particles vibrate -no expand upon heating - up IMF -down KE -up (3) PE

Distillation

-Separate two liquids by heating them - the liquid with the lowest boiling point is realized first -lighter pigment goes the farthest

Filtration

-Separation of two phases by particle size -filtrant- the collected substance -residue- what is left in the filter paper

chemical reaction

-a change occurs in which one or more reactants becomes one or more products with the formation of bones -reactants to products -compounds/molecules on both sides -coefficient -subscript

Chemical properties

-behavior/ability of substance to undergo a specific change -change will occur when substance is in contact with something else, another chemical agent

signs of chemical reaction

-bubbling/freezing -gas production -energy production/given off -precupitate -color change

chemical change

-change in composition -new substance -different properties then you started with -cannot be easily reversed -always accompanied by energy change (heat+sound)

Element

-homogenous -cannot be broken down simpler by physical or chemical means -atomic numbers -periodic tables -represented by one or two letters

Homogenous mixture

-identical composition throughout sample -unable to see individual parts -parts are equally distributed Example: lemonade, iced tea, sea water, toothpaste

Matter

-is all around us -can be identified by its physical or chemical properties -any substance regs takes up space (volume) and has mass

Gas

-no definite shape - g system expand to fill container - not dense - triple up KE plus up tempature becomes up KE - down PE - double down IMF weak attractive forces between paticles.

liquids

-no definite shape -definite volume -arrangement random, less tightly packed - less dense -a flow -down IMF, up KE, down PE

Heterogenous mixture

-non-uniform distribution -not equally distributes -can see parts -individual parts remain distinct Example: cole slaw, Mac and cheese, blood, granite, chicken soup

solids exhibit predictable behavior

-organization of particles -particle movement

Substance

-pure -matter that has same composition and constant properties

Chemical reaction

-reactants to product -compounds and molecules on both sides -coefficients -

Physical change

-rearrangement of particles making up sample -no change to identify of substance -no new substance -no change to chemical properties

Chromatography

-separation of a liquid mixture based on solubility -Round bottom flask over a bunts on burner -tube- condenser

Heat

Always mover high to low like diffusion depends on temp astute of two different points

Physical property

Color. Size. Shape. Texture. Density Pattern. Luster. State of matter. Composition Hardness. Mass. Volume. Smell. Freezing point Melting point. boiling point. Silubiloty. Attraction/repulsion. Viscosity. Ductility. Malleability. Brittleness. Conductivity Volatility

Extensive (physical property)

Depend on the amount of matter in sample (quantitative-numbers)

Intensive (physical property)

Depend on type of matter in sample (qualitative-descriptive)

Products

Formed at the end of reaction (listed right)

Mixture

Heterogenous combination of parts

Impure

Matter with varying composition

Tempature

Measure of average kinetic energy of particles

Atom

Most simple form of matter

Mixture

Physical blend of substance/components -physically separated -individual properties -no fixed ratio

Physical properties

Quality/characteristics that can be observed/measured without changing composition of matter

Decanting

Separate two liquids by the phases they are in (pouring off the lighter liquid)

irreversible (physical change)

cutting/cracking/filling (inability to return to original shape)

phases/states of matter

each phase has distinguishing characteristics

evaporation/boiling

energy is great and effects all particles of the system double up KE, own PE)

kinetic energy

energy of motion

chemical change examples

flammability/corrosiveness/rusting/cooking/reactivity/oxidation/neutralization/respiration/digestion

colliod

hetero. solution with medium sized particles

concentrated solutions

large solute dissolved

Plasma (state of matter)

made of electrons and ions of an element (example stars; lightening)

tempature

measure of average kinetic energy of particles

coefficients

numbers before formulas

subscript

numbers below line in formula

Chemical property

pH. Rusting. Burning. Rotting. Reactivity Toxicity. Radioactivity. Growing. Heat of combustion. Flamibilty. Chemical stability. Bond formation Oxidation state.

reversible (physical change)

phase change

dilute slutions

small solute dissolved

precipitate

solid formed in liquid

aquenous

substance dissolved in water

reactions

substances listed on left/start the reaction

products

substances listed on the right/ formed at the end of reaction

molecules

two atoms chemtically combined

diatomic molecules

two kinds of elements

alloys

two or more metals

heat

always move high to low like diffusion depends on tempature of two different points

Solution

Solute + solvent

Reactions

Start the reaction (listed left)

Chemistry

Study of matter -composition -structure -energy changes it goes through

Solute

Substance dissolved

Electrolysis

Two liquids are speared by a electric cure eg based on their polarity (charges)

Compound

Two or more elements chemically combined -original elemental properties lost -can be decomposed -electrically neutral -represented by chemical formula

Solvent

What solute is dissolved in