TEAS Chem

solid

definite shape & volume; closely packed/incompressible particles; high vibrational, low translational

liquid

indefinite shape (takes shape of container), definite volume; particles close and moving freely; moderate motion (incompressible)

gas

indefinite shape & volume; expands to fit any container; low vibrational, high translational (compressible)

plasma

“special gas” created by heat/electricity

state changes

can change if temperature changes

what does “heat absorbed” mean

increase in temperature and kinetic energy

kinetic molecular theory

1. matter is made of tiny particles

2. particles are in constant motion

3. higher temp = faster particle movement (kinetic energy)

intermolecular force of attraction (IMF)

particles are attracted to each other

IMF in solid

is higher is solid state (particles are more close together)

IMF in gas

is lower in gas state (instead they have higher kinetic energy)

condensation

gas to liquid (100 deg celcius)

sublimation

solid to gas

deposition

gas to solid

atom

building blocks of matter

elements

different types of atoms

periods

rows on periodic table = number of shells

groups

vertical columns on table = number of valence e-

elements in the same group/column

have similar chemical properties

metals on periodic table

end in -ium and are on left of the staircase

electronegativity

how capable an atom is of attracting a pair of electrons (increases as you go right of the table)

ionization

process where a neutral particle are ionized into a charged molecule (gain/lose electron)

covalent bonds

sharing of one or more electron btwn atoms

covalent bonds occurs

between atoms with similar electronegativity/between non metals

protons

determines element (EQUALS TO ATOMIC NUMBER)

mass number

number of protons and neutrons

atomic radius

highest at bottom left of table, lowest at top right

chemical property

substances combine/breakdown, chemical reactions, make something new

chemical property examples

rusting, burning

physical property

no chemical reaction (conduction, density, state changes)

density equation

density = mass / volume

extensive property

changes depending on amount of stuff (mass, volume, moles, length)

intensive property

doesn’t change depending on amount of stuff (color, specific heat, melting/freezing point, density)

single replacement reaction

a + bc = b + ac (cationic/anionic) - switching metals

double replacement rxn

ac + bd = ad + bc (substitution, ion exchange, metathesis) - inner combinem, outer combine

synthesis rxn

a + b = ab (release energy/exothermic)

decomposition rxn

ab = a + b (absorb energy/endothermic)

pH

changes between numbers is 10x

reaction rate

incr concentration, surface area, temp, pressure > incr number of collisions = incr rxn rate

le chateller’s principle

when stressor is applied to system, system will respond by offsetting stressor

adding concentration to one side of the equation

forwards reaction to other side to offset/restore equilibrium

removing concentration on one side of the equation

forwards reaction to side removed to balance/restore equilibrium

subshells

Save PDF - +4 every time you move up subshell

1 shell (k)

2 e- in shell

2 shell (L)

8 e- in shell

3 shell (M)

18 e- in shell

4 shell (N)

32 e- in shell

pressure and volume

have inverse relationship - incr volume = decr pressure vice versa

inc volume

= decr pressure, favors side with more moles

decr volume

= incr pressure, favors side with less moles

adhesion (h2o property)

binding btwn dissimilar molecule/surface

cohesion (h2o property)

attraction of h2o to other h2o; enhances surface tension of h2o

universal solvent

h2o can dissolve polar substances

homogenous mixture

a solution (mix of 1+ solutes dissolved in solvent) - uniform composition

heterogenous mixture

insoluble, non-uniform

molarity

number of moles of solute per 1 liter of solution

dilution

reducing concentration of solute in solution by adding more solvent

dilution equation

m1v2 = m2v2

neutralization reaction

when acid and bases react, forms salt and h2o

alcohol

c2h5oh

glucose

c6h12o6

exothermic reaction

heat is released on product side

exothermic reaction shifts rxn to…

left; rxn is reversed/away from heat

endothermic rxn

heat is absorbed on reactant side

endothermic reaction shifts rxn to…

right; rxn more forwards/away from heat

substrate

reactant that involves an enzyme

pH scientific notation

[H+] = 1.0 × 10^-4M

• remove negative.. pH = 4

buffers

substance that resist change in pH by absorbing extra H+/OH- ions

what are buffers made of

weak acid and weak base (neutralizes/maintains pH)

blood buffers

carbonic acid (weak acid) and bicarbonate (weak base)

ionic bond

metal and non-metal

ionic bond - electrons

transfer (gain/lose) electrons

ionic bond - metals

lose electrons (becomes cation)

ionic bond - non-metals

gain electrons (becomes anion)

atoms in column 4

do not make ions

1+ charges

Li+, Na+, K+

2+ charges

Mg2+, Ca2+

2- charges

S2-, O2-

1- charges

F-, Br-, Cl-

covalent bond

non metal and non metal

covalent bond - electrons

sharing electrons equally (non-polar) or non equally (polar)

triple bond

sharing 3 pairs of electrons (strongest and shortest)

solutes

can be gas, liquid, or solid

polar

can dissolve in h2o (salt, sugar, alcohol, nucleic acid, proteins)

non-polar

cannot mix in h2o (lipids)

how to distinguish non-polar

only C and H, only C and Cl, combo of C, H, Cl, made of two same atom (N2)

octet rule

atoms want to have 8 electrons to be stable (inert)

density

D = mass (g) / volume (cm²)

water displacement

finding volume of irregular object by putting it in water (difference in water vol)

polar bonds

slightly pos/neg charge on diff sides/e- shared unequally

nonpolar bonds

no partial charges/electrons shared equally

distinguishing nonpolar bonds

C-H and C-C bonds, C-Cl, C-H-Cl, diatomic elements (N2)

groups 3-12

transitional metals

group 9

halogens

group 10

noble gases

group 1

alkali metals

group 2

alkaline metal

conductors

allows heat/electricity to flow freely (metal)

insulators

block the flow heat/electricity (non-metals)