Dr. Chu Baylor CHE 1301- Test 1

physical properties

ex: color, shape, melting point, density, dissolving, mass, volume

characteristics that can be observed without changing composition

chemical properties

ex: flammable, corrosive, oxidizer

characteristics that may only be observed/measured through chemical reaction

extensive properties

depends on the amount of material measured

intensive properties

does not depends on the amount BUT on the nature of the material

deci

10^ -1

centi

10^ -2

milli

10^ -3

micro

10^ -6

nano

10^ -9

pico

10^ -12

mega

10^6

kilo

10^3

deka

10^1

hecto

10^2

giga

10^9

Molecule

two or more atoms joined and act as a unit

chemical reaction

one substance changes to another by recognizing the way the atoms are attached to each other

theory

a model for the way nature is and tries to explain no merely what nature does, but why and is based on thorough study

robert boyle

Who was the first "chemist"?

-pressure and air

mass is neither created nor destroyed

law of conservation of mass

ex: the total mass of substances does not change during a chemical reaction

Law of definite proportions

a given compound always contains exactly the same proportion of elements by mass (Joseph Proust)

law of multiple proportions

when two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers

J.J. Thomson

Who discovered the electron?

charge to mass ratio of an electron

1.76 x 10^8 C/g

mass of an electron

9.11 x 10^-31 kg

high

beta particles have high/low speed electrons?

twice, opposite

alpha particles possess a charge ___ that of the electron but with the ___ sign

Plum-Pudding model

Ernest Rutherford proves what experiment wrong?

positive

The foil experiment created a nuclear model of an atoms and realized that the nucleus was ____

Composition of an atom

an electrically neutral atoms, spherical entity composed of a positively charged central uncles surrounded by one or more negatively charged electrons

Isotope

same element with atoms of different masses

identical

isotopes show ___ chemical properties

electrons

chemistry of an atom is based on the # of ___

cations

the removal of an electron making an atom positive

anions

the addition of an electron making an atom negative

wavelength (lambda)

-horizontal

distance between two peaks or troughs in a wave

amplitude (A)

-vertical

height of wave from center to peak or trough

frequency (v)

number of waves that pass a particular point in 1 sec

speed (c)

wavelength x frequency

Higher wavelength =

shorter frequency

speed of light (c)

2.9979 x 10^8 m/s

1nm = ?m

1 x 10^ -9

1m = ?nm

1 x 10^9

frequency (v) = x/x

c ÷ wavelength

color of light is determined by?

wavelength or frequency

shorter wavelength =

higher frequency

what light has the lowest energy?

radiowave

what light has the highest energy?

gamma ray

plancks constant (h)=

6.626 x 10^-34 J*s

hv= x/x

hc ÷ wavelength

E=mc^2 factored

m=E/c^2 , hc/Wl ÷ c^2 , h/(WL*c)

wavelength (lambda) =

h ÷ mv

quantized means-

that the atom could only have specific amount of energy

n=1 orbit is classified as the

ground state

an atom is less/more stable in an excited state

less

E =

-2.178x10^-18J(Z^2/n^2)

The bohr model only works for?

hydrogen

the wave and particle nature of an electron are ______ properties as you know more about one you know less about the other

complementary

Who developed quantum mechanics?

Erwin Schrodinger

Probability of finding an electron at a particular position is greater near the ?

nucleus

volume of the spherical shell _____ with distance from the nucleus

increases

principal quantum number (n)

size and energy

angular momentum quantum number (l)

shape

magnetic quantum number (ml)

orientation of the orbital in space

spin quantum number (ms)

spin of the electron

the principal quantum number (n) can be any number ____

greater than 1

the angular momentum quantum number (l) can be any integer from 0 to

n-1

s orbital shape

spherical

p orbital shape

dumbell

d orbital shape

four-leaf clover

f orbital shape

odd combinations

l=0

s

l=1

p

l=2

d

l=3

f

the number of nodal surfaces ___ as n increases

increases

how many p orbitals are there in every sub shell?

3

p orbital (l=1) ml=?

-1, 0, 1

s orbital (l=0) ml=?

0

how many f orbitals are there in every sub shell?

7

electron spin possible value

plus/minus 1/2

each orbital can hold ___ electrons

2

pauli exclusion principle

no more than 2 electrons per orbital

degenerate orbitals

for one-electron hydrogen atom, orbitals on the same energy level have the same energy

polyelectronic atom

this atoms with more than one electron

Aufbau principle

energy level and sub levels fill from lowest energy to high

Hund's rule

when filling orbitals that have the same energy, place one electron in each before completing pairs

triads

groups of three elements that have similar properties

diamagnetic

element with no unpaired electrons

paramagnetic

element with unpaired electrons

1A

alkali metals

2A

alkali earth metals

7A

halogens

8A

noble gases

The group number on the periodic table indicates the number of ___?

valence electrons

s orbital maximum # of electrons

2

p orbital maximum # of electrons

6

d orbital maximum number of electrons

10

f orbital maximum # of electrons

14

are metals cations or anions?

cations- lose elctrons