Modern Atomic Theory Ws #2

name:______date:______period:_____

modern atomic theory ws #2

i. completion

1. any orbital, regardless of type, may contain a maximum of ______electrons.
2. the fact that no two electrons in the same atom can have the same set of four quantum numbers is known as ______.
3. the two possibilities for electron spin are ______and ______.
4. not pairing electrons within a sublevel until necessary is known as ______.
5. n s2, n p5 is the characteristic outer energy level electron configuration of the group ______elements.
6. in the lewis dot system, the nucleus and inner energy level electrons are represented by the ______of the element and are usually called the ______.
7. the maximum number of electrons allowed in the n=4 main energy level is ______.
8. the outer energy level electrons are known as ______electrons.
9. there are ______possible orientations for the d orbitals.
10. when all the electrons in an atom are in the lowest possible energy state, the atom is said to be in the ______.
11. an orbital pair of electrons differ only in ______.
12. in any p sublevel there are ______p orbitals.
13. the number of orbitals in the outermost energy level of neon is ______.
14. if an electron has absorbed energy and has shifted to a higher energy level, the electron is said to be ______.
15. each orbital in a sublevel must contain one electron before any orbital in the sublevel can contain ______.
16. the electron configuration, 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p1, is that of the element ______which contains ______valence electrons.
17. if n=3, the total number of orbitals is ______, and the number of d orbitals is ______.
18. a sublevel designated 4p means a p sublevel in the ______main energy level.
19. the number of electrons in the kernel of chlorine is ______.
20. ______attributed significant wave properties to small, fast-moving particles such as electrons.
21. [Ne] is called the “______” and represents the first ______electrons in an atom.

ii. true or false

_____ 1. it is not possible to determine the path of an electron in an atom.

_____ 2. in the modern atom, bright line spectra are still accounted for through certain allowed energy transitions of electrons.

_____ 3. an orbital pair of electrons may differ in ms value.

_____ 4. a d sublevel can hold a maximum of 14 electrons.

_____ 5. in the modern atom, the electron is pictured in terms of probability.

_____ 6. some orbitals contain more than two electrons.

_____ 7. all electrons are identical.

_____ 8. an orbital is a volume in space where the electron is located ~90%+ of the time.

_____ 9. the modern atom is sometimes thought of as a small positive nucleus surrounded by a cloud of negative charge.

_____ 10. for all s electrons l and ml are both equal to zero.

_____ 11. the process of placing electrons in the lowest possible energy positions in order to obtain ground state configurations for atoms is known as “the aufbau principle”.

_____12. the wave mechanical or quantum mechanical model of the atom applies equally well to one- and multi-electron systems.

_____ 13. it is impossible to draw a reasonable likeness of an atom.

_____ 14. positive spin ( ) refers to an electron that is spinning clockwise.

_____ 15. [Xe] 5s2 is the electron configuration for Sr.

iii. periodic table cheat sheet

write the sublevel being filled between arrows, i.e. 2p, 4s, 5f, etc.

iv. more fun!!!!!

1. identify the elements whose atoms have the following configurations:

1. 1s2 2s2 2p3
2. 1s2 2s2
3. [Ne] 3s2
4. [Ne] 3s2 3p3
5. [Ar] 4s1
6. [Ar] 3d6 4s2

1. is it possible to define the exact path of an electron around a nucleus? what principle do we rely on to answer this question?
2. what sublevel fills after the 6p? after the 4d? after the 6s?
3. what element has the following quantum numbers?

1. 4, 0, 0, -½
2. 2, 1, -1, +½
3. 3, 2, 0, -½
4. 2, 1, +1, +½
5. 3, 2, -2, -½
6. 4, 1, -1, +½

1. in which orbital does the electron have the greatest energy?

1. 1s or 2s
2. 2s or 2p
3. 3s or 3d

1. write quantum numbers for the following electrons

1. 3s1
2. 2p5
3. 2p2
4. 3d4
5. 3d7
6. 4p5

1. how many electrons can be accommodated in the following:

1. a d orbital
2. a p sublevel
3. all n=3 orbitals

1. which orbitals cannot exist according to the modern atomic theory? 6h, 4g, 5h, 7j
2. what are valence electrons?
3. what is the lewis dot structure for iodine? how many electrons does the kernel represent?

v. complete the following table of quantum numbers for the last electron entered.

In