Periodic Trends in Atomic Structure: Ionization, Electron Affinity, and Electronegativity
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36 Terms
What is the atomic radius trend across a period?
The atomic radius decreases.
What is the atomic radius trend down a group?
The atomic radius increases.
What is ionization energy?
The amount of energy required to remove the most loosely bound electron of a gaseous atom.
What causes electron shielding?
The presence of other negatively charged electrons between the outer electron and the nucleus.
Which electrons are shielded the most?
Electrons in the 2 energy level.
What is the trend for ionization energy across a period?
Ionization energy increases.
What is the trend for ionization energy down a group?
Ionization energy decreases.
Does aluminum follow the general trend for ionization energy across the periodic table?
No.
What is the electron configuration for aluminum?
1s² 2s² 2p⁶ 3s² 3p¹.
Why does aluminum have a lower ionization energy than magnesium?
Aluminum has more shielding affecting the 3p electron.
Does oxygen follow the general trend for ionization energy across the periodic table?
No.
What is the orbital notation for oxygen?
1s² 2s² 2p⁴.
Why does oxygen have a lower ionization energy than nitrogen?
Oxygen has unevenly shared orbitals causing repulsion.
What is the first ionization energy?
The energy required to remove the first electron from a neutral atom.
What happens to successive ionization energies?
They increase.
What is true about the ionization energy of any atom that is isoelectronic with a noble gas?
It has high ionization energy due to the stability of the noble gas configuration.
What is electron affinity?
The energy change when an electron is added to a neutral atom.
What does a negative sign on electron affinity indicate?
It indicates that energy is released when an electron is added.
What is the trend for electron affinity across a period?
Electron affinity becomes more negative.
What is the trend for electron affinity down a group?
Electron affinity becomes less negative.
Which element is easier to gain an electron: element X with -200 kJ/mol or element Y with -250 kJ/mol?
Element Y.
Why does nitrogen have an electron affinity of 0 kJ/mol while carbon has -126.3 kJ/mol?
Due to differences in their orbital notations.
Define cation.
A positively charged ion due to the loss of electrons.
Define anion.
A negatively charged ion due to the gain of one or more electrons.
Which elements tend to form cations?
Metals.
Which elements tend to form anions?
Non-metals.
What are valence electrons?
Electrons in the outermost energy levels.
What is the trend for valence electrons across a period?
The number of valence electrons increases.
What is the trend for valence electrons down a group?
The number of valence electrons remains the same.
Define electronegativity.
The ability of an atom in a chemical compound to attract electrons.
What is the trend for electronegativity across a period?
Electronegativity increases.
What is the trend for electronegativity down a group?
Electronegativity decreases.
Why are some noble gases not assigned electronegativities?
They do not form compounds.
What is the most electronegative element on the periodic table?
Fluorine.
What is nuclear charge?
The total charge of the nucleus due to protons.
What is electron shielding?
The effect of inner electrons reducing the effective nuclear charge felt by outer electrons.
