26. What is an orbital and how is it similar to a Bohr orbit? 3pts
An orbital is a 3 dimensional region of space where an electron is most likely to be found. Each
orbital differs in size, shape, and orientation. It is similar to the Bohr orbit because of its quantum
nature. It takes a specific amount of energy to move between energy levels in the Bohr model and it
takes specific amount of energy to move between orbitals.
b) How is an orbital different than a Bohr model orbit? 3pts
An orbit is a defined path while an oribital is a region of space that there is a probability of finding
an electron. One orbit differs from another orbit by its radius, while orbitals differ in size, shape
and orientation. There are seven Bohr orbits while there are over twenty orbitals. Orbits are 2 D
and orbitals are 3D.
c) How does a 3px orbital differ from a 3py orbital? 2pts
A 3px orbital is oriented on the x axis and while a 3py orbital is oriented on the y axis
d) How does a 1s orbital differ from a 3s orbital? 2pts
The spherical s orbitals have different sizes. A 3s orbital has a larger volume than a 1s orbital
e) How does a 4px orbital differ from a 4s orbital? 2pts
A 4px orbital has a dumbbell shape oriented on the x axis while the 4s orbital has a spherical shape
oriented symmetrically around the nucleus.
27.
What property of an electron determines the orbital an electron is found in?
a) The energy of the electron
b) The size of the electron
c) The charge on an electron
d) The rotation of an electron
e) None of the above
28.
In order for an atom to have the following electron configuration what must have happened
to this atom? What will eventually happen to this atom? 3pts
1s2 2s2 2px2 2py2 2pz 3s2 3px 2 3py2 3pz 2 4s2 3dxy2 3dxz2 3dyz 2 3dx2-y22 3dz22 4px2 4py2 4pz2
5s2 4dxy2 4dxz 24dyz2 4 dx2-y22 4dz22 5px1 5py1 5pz1 6s1 4f1 4f2 4f3 4 f4 4f5 4f6 4f7 5dxy 5dxz5dyz 5dx2-y2 5dz2
6px 6py 6pz 7s
This electron configuration represents an atom in the excited state. Therefore energy must have
been absorbed by this atom. Eventually the electrons will return to lower energy levels. In the
process of returning to lower energy levels the electrons will release a “light” characteristic of that
energy transition
29. What electron transition of lead will involve the highest frequency photon and why? 2pts
a) 6s --> 5px
b) 6s ---> 4dz2
c) 6s  3py
d) 6s  4py
Why? The larger the energy drop according to the energy associated with the sequence of
orbitals the higher the frequency photon released. High energy photons have high
frequencies.
30. What electron transition of lead will involve the lowest frequency photon and why? 2pts
a) 5py  6s
b) 4dz2  6s c) 3py  6s
d) 4py  6s
Why? The smaller the energy transition according to the energy associated with the
sequence of orbitals the lower the frequency photon released. Low energy photons have low
frequencies.
31. The energy of a photon 1pt
a. It is directly related to speed of the photon
b. It is directly related to the number of photons released
c. It is directly related to speed of reindeer
d. It is directly related to frequency of the photon
e. It is directly related to the frequency.
32. a) What atom has the following electron configuration? 1pt Mo
1s2 2s2 2px2 2py2 2pz2 3s2 3px 2 3py2 3pz 2 4s2 3dxy2 3dxz2 3dyz 2 3dx2-y22 3dz22 4px2 4py2 4pz2
5s1 4dxy1 4dxz 14dyz1 4 dx2-y21 4dz21 5px 5py 5pz 6s 4f1 4f2 4f3 4 f4 4f5 4f6 4f7 5dxy 5dxz5dyz 5dx2-y2 5dz2
6px 6py 6pz 7s
b) What type of stability does this atom have? full shell stability or half shell stability or
noble gas stability – Explain 2pts
Half shell stability – the 4d orbitals each have one electron in them – the sublevel is half full.
An electron that “normally” would be found in the 5s has moved to the 4d to create that half shell
stability.
33. a) What is the electron configuration of Cesium?
55Cs
3pts
1s2 2s2 2px2 2py2 2pz2 3s2 3px 2 3py2 3pz 2 4s2 3dxy2 3dxz2 3dyz 2 3dx2-y22 3dz22 4px2 4py2 4pz2
5s2 4dxy2 4dxz2 4dyz2 4 dx2-y22 4dz22 5px2 5py2 5pz2 6s1 4f1 4f2 4f3 4 f4 4f5 4f6 4f7 5dxy 5dxz5dyz 5dx2-y2 5dz2
6px 6py 6pz 7s
b) What is its short hand electron configuration of cesium? 2pts
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1 4f 5d 6p 7s 5f 6d 7p
c) What is its short hand electron configuration of cesium? 3pts
] 6s1
[ kr
d) What is the electron dot diagram of cesium? 2pts Cs
34. a) What atom has the following electron configuration? 1pt Se
1s2 2s2 2px2 2py2 2pz2 3s2 3px 2 3py2 3pz 2 4s2 3dxy2 3dxz2 3dyz 2 3dx2-y22 3dz22 4px2 4py1 4pz1
5s 4dxy 4dxz 4dyz 4 dx2-y2 4dz2 5px 5py 5pz 6s 4f1 4f2 4f3 4 f4 4f5 4f6 4f7 5dxy 5dxz5dyz 5dx2-y2 5dz2
6px 6py 6pz 7s
b) What is its short hand electron configuration of this atom? 1pt
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
c)What is its short hand electron configuration of this atom? 2pts
[ Ar
] 4s2 3d10 4p4
d) What is the electron dot diagram of this atom? 2pts
35
Use the electron dot diagrams of the cesium atom from question 33 and the atom from question
34 to show how the two atoms would bond. 5pts
-2
Cs
Cs
Se
Se
Cs+1
Cs+1
Se
36. Use electron dot diagrams to show the reaction between Barium (Ba) atoms and Nitrogen (N) atoms.
You may need multiple atoms of each to complete the diagram.
15 N has 7 protons 7 electrons and 8 protons
Ba is in the s block and N is in the p block
7
Ba
N
Ba+2
N
Ba+2
-3
N
N
-3
Ba
Ba+2
Ba
Ionic
Types of Bonds
Metallic
Covalent – Nonpolar / Polar
37. What type of bond is characterized by the nucleus of one atom’s attraction for a second atom’s
electron and the nucleus of the second atom’s attraction for the first atom’s electron
Covalent 1pt
38. What type of attraction occurs between oppositely charged particles that are formed as a result of a
transfer of electrons between atoms.
Ionic1pt
39 What type of bond forms between Hydrogen (H) and Bromine (Br) and how did you determine this?
3pts
nonmetal to nonmetal = covalent
3.0 – 2.2 = .8 electronegativity difference from the periodic table on the 1st page of the test=polar
POLAR COVALENT
40 Which of the following bond because loosely held electrons form a sea of mobile electrons which
hold the rest of the atom ( essentially a positive ion ) in a regular geometric pattern 1pt.
a) Titanium (Ti) to (Ti)
b) Phosphorous (P) to (P)
c) Iodine (I) to (I)
d) Xenon (Xe) to (Xe)
41. What type of bond forms between potassium (K) and chlorine (Cl) and how did you determine this?
2pts
Metal to nonmetal = transfer of electrons = ionic bond
42. This type of bond is found between hydrogen and oxygen atoms found in methanol CH3OH (l) and
how did you determine this? 3pts
nonmetal to nonmetal = covalent
3.5 – 2.2 = 1.3 electronegativity difference from the periodic table on the 1st page of the test=polar
POLAR COVALENT
43. What type of bond is found between silver atoms ( Ag ) in a silver chain and how did you determine
this? 2pts
Metallic because Ag is a metal combined to itself
44. What type of bond will form between hydrogen atoms and phosphorous atoms and how did you
determine this? 3pts
nonmetal to nonmetal = covalent
2.2 – 2.2 = 0 electronegativity difference from the periodic table on the 1st page of the test=non-polar
NONPOLAR COVALENT
45. Which of the following has the largest atomic radius? 1pt
a) Rubidium b) Cesium c) Strontium d) Barium e) Bromine f) Krypton g) Tellurium h) Iodine
Rb
Cs
Sr
Ba
Br
Kr
Te
I
bottom left metal
46. Which of the following would require the most energy to remove an electron and have the highest
attraction for electrons? 1pt
a) Rubidium b) Cesium c) Strontium d) Barium e) Bromine f) Krypton g) Tellurium h) Iodine
Rb
Cs
Sr
Ba
Br
Kr
Te
I
upper right nonmetal that is unstable
47. How does the atomic radius, ionization energy required, and electronegativity vary as you move
across period 5 from Rubidum (Rb) to Xenon (Xe)? How does this effect the tendency of
electrons ability to lose gain or share electrons? 4pts
The radius decreases which causes the ionization required to increase, electronegativity to increase
which then causes a tendency to share / gain electrons
48. How does the atomic radius, ionization energy required, and electronegativity vary as you move
down from C to Si to Ge to Pb? How does this effect the nonmetallic / metallic properties of these
atoms? 4pts
The radius increases which causes the ionization required to decrease, electronegativity to decrease
which then causes a tendency to lose electrons and become more metallic in nature
49. Which of the following will not conduct electricity as a solid and when dissolved in water? Why?
2pts
a) MgCl2 b) C6H12O6 c) KI d) Ag
Ionic compounds composed of a metal to a nonmetal will dissociate in water to form positive and
negative ions capable of conducting electricity
50 Which of the following will not conduct electricity as a solid and will conduct when dissolved in
water? Why?
2pts
a) MgCl2 b) C6H12O6 c) KI d) Ag
Nonmetal to nonmetals form covalently bonded molecules that do not dissociate in water to form
positive and negative ions capable of conducting electricity