Chemistry chapter 4
noble gases
group 18 elements, helium, neon, argon, krypton, xenon and radon
where do electrons exist?
in orbitals
when current is passed through a gas at a low pressure, the potential energy of some of the gas atoms _______
increases
for electromagnetic radiation, as the wave length of light decreases, the frequency ____, which means its ____ proportional
increases, inversly
spin quantum number
indicates the two fundamental spin states of an electron in an orbital
how does the quantum model improve on the bohr model?
it describes the arrangements of electrons in atoms other than hydrogen
what was the major shortcoming of Rutherford's model of the atom?
it didnt explain how the atoms negatively charged electrons occupy the space sorrounding the nucles
the heisenburg uncertainty principle
it is impossible to determine simultaneously both the position and velocity of an electron or any other particle
write both the complete electron-configuration notation and the noble-gas notation for a rubidium atom
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 5s^1. [Kr] 5s^1
without looking at the periodic table, write the complete electron configuration for the element with atomic number 25
1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^2
an orbital with two electrons is represented with an arrow pointing up and an arrow pointing down. what does that show about the electrons?
they are paired and have opposite spins
photon
partical of electromagnetic radiation carrying a quantum of energy
what is the elctron configuration if there is 5 electrons?
/1s /2s /2px /2py /2pz
name how many electrons orbitals1-4 can hold
1. 2 2. 8 3. 18 4. 32
how many electron-containing d orbitals are there in an atom of tin? name the element in the 4th period whose atoms have the same number of highest-energy-level elctrons as tin
10, germanium
what does notation in the 2nd period look like
1s^blank 2s^blank 2p^blank
how many electron-containing orbitals are in an atom of iodine? how many of these orbitals are filled? how many unpaired electrons are there in an atom of iodine?
27, 26, 1
identify the elements in the second, third, and fourth periods that have the same number of highest-energy level electrons as rubidium
2nd: lithium Li 3rd: sodium Na 4th: potassium, K
all forms of electromagnetic radition move at a constant speed of
3.0 x 10^8 m/s
the electron configuration of boron is 1s^2 2s^2 2p^1. how many electrons are present in an atom of boron? what is the atomic number for boron? write the orbital notation for boron.
5 electrons present. the atomic number is 5. up arrow, down arrow/1s up arrow, down arrow/2s up arrow/2px /2py /2pz
the electron configuration of nitrogen is 1s^2 2s^2 2p^3. how many electrons are present in an atom of nitrogen? what is the atomic number for nitrogen? write the orbital notation for nitrogen.
7 electrons present. atomic number is 7. up arrow down arrow/1s up arrow down arrow/2s up arrow/2px up arrow/2py up arrow/2pz
the electron configuration of flourine is 1s^2 2s^2 2p^5. what is the atomic number for flourine? how many of the p orbitals are filled? how many unpaired electrons does a flourine atom contain?
9, 2, 1
identify the elements in the 6th period that have one unpaired electron in their 6s level
Au, Cs, and Pt
what does notation in the 4th period look like
[Ar]4s^blank or [Ar] 3d^blank 4s^blank 4p^blank
write the noble-gas notation for tin, Sn. how many unpaired electrons are there in an atom of tin?
[Kr] 4d^10 5s^2 5p^2. 2
what does notation in the 5th period look like
[Kr] 5s^blank or [Kr]4d^blank 5s^blank 5p^blank
what does notation in the third period look like?
[Ne] 3s^blank and if more, [Ne]3s^blank3p^blank
write the noble-gas notation for a gold atom
[Xe] 4s^14 5d^10 6s^1
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
electromagnetic spectrum
all the forms of electromagnetic radiation for the electromagnetic spectrum
aubau principle
an electron occupies the lowest energy orbital that can recieve it
how many electron-containing orbitals are in an atom of iron? how many of these orbitals are completely filled? how many unpaired electrons are there in an atom of iron? in which sublevel are the unpaired elctrons located?
an iron atom has 15 orbitals. eleven of these orbitals are filled. there are four unpaired electrons. they are located in the 3d sublevel
what did plank propose?
an object emits small amounts of electromagnetic energy
noble gas configuration
an outer main energy level fully occupied, in most cases, by eight electrons
what are the three basic rules for electron configuration?
aufbau principle, pauli exclusion principle, and hunds rule
why is this true: it is impossible to determine simultaneously both the position and velocity of an electron or any other particle
because any attempt to locate a specific electron with a photon knocks the electron off course
quantum theory
decribes mathmatically the wave properties of electrons and other very small particles
when an excited atom returns to its ground state, how does it give of its energy it gained?
electromagnetic radiation
write both the complete electron-configuration notation and the noble gas notation for iodine, I. how many inner-shell electrons does an iodine atom contain?
electron configuration notation: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 5s^2 5p^5. noble gas notation: [Kr] 4d^10 5s^2 5p^5. contaions 46 inner shell electrons
write both the complete electron-configuration notation and the noble-gases notation for iron, Fe
electron-configuration: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 4s^2 the noble gas notation: [Ar] 3d^6 4s^2
how do you build electron configurations for the ground state of any particular atom
energy levels of the orbitals are determined. then electrons are added to orbitals one by one
the energy of a photon depends on the
frequency of the radiation
pauli exclusion principle
no 2 electrons in the same atom can have the same set of 4 quantum numbers
hunds rule
orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a 2nd electron, and all electrons in singly occupied orbitals must have the same spin
each particle of light carries a _____ of energy called ______
quantum, photon
orbital
region around the nucleas that indicates the probable location of an electron
the significant feature of wave motion is its ____ nature, which can be characterised by the measurable properties of _____ and _____
repetitive, wavelength, frequency
quantum numbers
specify the properties of atomic orbitals and the properties of electrons in orbitals
angular momentum quantum number
symbolized by l, indicates the shape of the orbitals
magnetic quantum number
symbolized by m, indicates the oriantation of the orbital around the nucleas
principal quantum number
symbolized by n, indicates the main energy level occupied by an electron
electron configuration
the arrangement of electrons in an atom
wavelength
the distance between corresponding points on adjacent waves
highest occupied level
the electron-containing main energy level with the highest principal quantum number
inner-shell electrons
the electrons that arent in the highest occupied energy level
the photoelectric effect
the emission of electroms from a metal when light shines on a metal
describe the bohr model of the hydrogen atom
the farther away the electrons where from the nucleas, the more energy it had
ground state electron configuration
the lowest energy arrangement of the electrons for each element
what is an atoms ground state
the lowest energy state
quantum
the minimal quantity of energy that can be lost or gained by an atom
frequency
the number of waves that pass a given point in a specific time
how is fequency expressed
waves/second
what is an atoms excited state
when an atom has a higher potential energy than it does in its ground state
when is the energy in an electron higher on its orbits?
when the orbits are farther away from the nucleas
if an orbital containing one elelectron is represented by a arrow pointing up, how is an orbital with two electrons represented?
with an arrow pointing up and an arrow pointing down
example of electromagnetic radiation
x rays, microwaves, radio waves
