Chapter Review

3. State the Pauli exclusion principle.
“In a closed system, no two electrons can occupy the same state”
6. What is a line-emission spectrum?
It’s the result of a released photon.7. Define ground state.
Conditions of atoms when they are in a low energy leveñ.
8. Define mole.
Molecular weight of a substance.
10. What is an orbital?
Its a wave functiondescribing the state of a single electron in an atom
19. How would you use the aufbau principle when you create an electron configuration.
To know the order in which orbitals are filled.21. Why can a p sublevel hold six electrons while sublevel s can hold no more than two electrons.
Because it has 3 sublevels in different angles so 3*2=6
23. How are the frequency andwavelength of light related?
Les frequency=More wavelength, More frequency=Les Wavelength
26. What is a mole? How is a mole related to Avogadro’s number?
MOL=Molecular weight of asubstance, Avogadro’s number is the number of particles found in a mole.
38. Write the electron configuration for nickel, whose atomic number is 28. Remember that the 4s orbital has a lowerenergy than the 3d orbital does and that the d sublevel can hold a maximum of 10 electrons.
1s^2---2s^2---2p^6---3s^2---3p^6---4s^2---3d^8
40. How many orbitals are completely filledin an atom that has 12 electrons?
1s^2--2s^2--2p^6-- 3s^2. 4
51. What is the electron configuration of zinc?
1s^2---2^2---2p^6---3^s2---3p^6---4s^2---3d^10
66. An advertising signgives off red and green light.
Which light has a higher energy? Green
One of the colors has a wavelength of 680nm and the other has a wavelength of 500. Which color has whichwavelength? Red=680nm Green=500nm
73. Which has more atoms: 3.0 g of iron, Fe, or 2.0 grams of sulfur, S?
Fe

.Myers, Thomas (2006) Holt Chemistry, Rinehart and Winston, Pgs.107-109