chemistry ch. 5 test review flashcards

the product of the frequency and wavelength equals

speed of the wave

because C, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is

inversely proportional to wavelength

according to the photo electric effect, certain kinds of light cannot eject electrons from metals due to the energy of light being too low

true

if electromagntic radiation A has a lower frequency then electromagnetic radiation b, then compared to b wavelength a is

longer

distance between two sucessive peaks in waves

wavelngth

quantum of electromagnetic energy is

photon

energy of photon is related to its

frequency

the emission of electrons from metals that have absorbed photons is called

photoelectric effect

a line spectrum is produced when an electron moves from one energy level to another

to a lower energy level (thing weird shaped ladder)

for an electron in an atom to change from the ground state to an excited state

energy must be absorbed

where do electrons circle the nucleus

in speicific allowed orbitals

emitting energy

go down energy levels (e.g 4 to 1)

absorbing energy

go up energy levels (e.g 2 to 3)

the electron in a hydrogen atom has its lowest total energy when the electron is in its

ground state

french scientist louis broglie theorized that

electrons could have a dual wave particle nature

three dimensional region around a nucleus where an electron may be found is called an electron path

false

according to the quantum theory of an atom, in an orbital

an electrons position cannot be known exaclty (think the rat and flashlight anaology)

main energy levels of an atom are indicated by the

principal quantum theory

number of sublevels within each energy level of an atom is equal to the value of

principal quantum theory

an electron for which n=4 has more energy than an electron that has n=2

true

the spin quantum number indicates that the number of possible spin states for an electron is an orbital is

2

the set of orbtil that are speherical shaped are directed along the x,y,and z axes are called

s orbitals

the major differences between a 1s orbital and a 2s orbital is that

the 2s orbital is at a higher energy level

the p orbital shape

dumbell

for s sublevel, number of orbital is

7

how many electrons can occupy the p orbital at each energy level

6 if they have opposite spins

if n is the principal quantum number of the main energy level, the max number of electrons of that energy level is

2n^2

how many electrons are needed to completly fill the fourth energy level

2n^2=2(4)^2=32

at n=1 the total number of electrons that can be found

2

the main energy level that can hold only two electrons is the

first

which of the following rules requires that each o the p orbitals at a paticular energy level recieve one electron before any of them can have two electrons

hunds rule

two electrons in the 1s orbital must have different spin quantum numbrs to satisfy

the pauli's exclusion principle

the sequence in which enregy sublevels are filled is specified by

the aufbau principle (bottom-top)

the aufbau principle states that an electron

occupies the lowest available energy level

what is the electron configuration for nitrogen atomic number 7

1s^22s^22p^3

the electron for aluminum atomic number 13 is

1s^22s^22p^63s^23p^1

according to bohr electrons cannot reside

in-between orbitals

with a wavelegnth of 170 nm what is the frequency in hertz of this particular wavelength of uv light

c=(wavelength)(v)=1.76x10^-14 hz

the electron configuration for nitrogen is 1s^22s^22p^3 what does the 3 in 2p^3 mean

electron

what is the relationship between wavelength and frequency

inversely proportional