AP Chemistry : Mass Spectroscopy of the Elements
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Example Questions
Example Question #11 : Mass Spectroscopy Of The Elements
What is the formal charge on the N atom in the [NH4]+ ion?
2
1
0
-1
1
N has 5 valence electrons. In the ion, N has 4 bonds, and thus 8 bonding electrons and 0 nonbonding electrons. Thus, formal charge = 5- (1/2)*8 - 0 = 1.
Example Question #41 : Atomic Structure And Properties
Which of the following ions or atoms is isoelectronic with neon?
O2-
Cl-
Mg
Na
O2-
Neon has an electron configuration of 1s22s22p6, just like O2-. Sodium has one extra electron, while magnesium has two extra electrons, beyond the neon configuration. Finally, the electron configuration for Cl- is 1s22s22p63s23p6. It is one period below flourine; F- would be isoelectric with neon.
Example Question #13 : Mass Spectroscopy Of The Elements
Which of the following orders the given elements in terms of increasing electronegativity?
Electronegativity increases moving from the left side of the periodic table to the right, and decreases moving down through a group (Excluding the Group 18 noble gases).
Thus the correct answer is 
Example Question #11 : Mass Spectroscopy Of The Elements
Which of the following ranks the acids from strongest to weakest?
Charge stability of halide ions increases with increasing atomic size (
This is not to be confused with electronegativity trends, which would predict the ordering of acids opposite the correct answer.
Atomic size (and thus the propensity to release protons (
This trend is tue, however, keep in mind that 
Example Question #42 : Atomic Structure And Properties
Anionic atoms are __________ than their respective neutral atoms because they have __________ electron(s) than their neutral atoms.
smaller . . . more
larger . . . more
smaller . . . less
larger . . . less
larger . . . more
Anions have at least one more electron than their neutral atoms. Adding an electron creates a shielding effect on other electrons in the same shell, decreasing the nuclear charge felt by each valence electron. As a result, the electrons will lie slightly further from the nucleus, corresponding to an increase in atomic radius. If there are no other electrons than the newly added electron in the valence shell, then the added electron was added to the now highest shell, which would significantly increase the size of the atom.
Example Question #41 : Atomic Structure And Properties
Which of the following is a cation?
A cation is a positively charged ion; calcium is the only species of the answer choices that has a positive charge. Negatively charged ions, such as the fluoride ion are known as anions.
Example Question #17 : Mass Spectroscopy Of The Elements
Which of the following is an isotope of Fluorine-20
isotopes have more neutrons, but their protons are the same
Example Question #41 : Atomic Structure And Properties
Which of the following contains the most neutrons?
Carbon-12
Boron-12
Nitrogen-14
Carbon-14
Oxygen-15
Carbon-14
The number following the compound is the isotope number, giving the number of protons and neutrons the element contains per atom. To get the number of neutrons you take the isotope number and subtract the atomic number of that element.
Example Question #13 : Mass Spectroscopy Of The Elements
Which of the following is NOT an isotope of oxygen
oxygen-14
14O
O2
O2-
oxygen- 16
O2-
O2- is an ion, and not an isotope; an isotope has the same number of protons and electrons, but a different number of neutrons
Example Question #11 : Mass Spectroscopy Of The Elements
Which of the following isotopes has the greatest number of neutrons?
Carbon-14
Nitrogen-13
Boron-10
Oxygen-15
Fluorine-16
Carbon-14
Carbon-14 has 8 neutrons
Nitrogen-13 has 6 neutrons
Oxygen-15 has 7 neutrons
Fluorine-16 has 7 neutrons
Boron-10 has 5 neutrons
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