Atomic Radius
What is the trend of atomic radius across a period (from left to right) on the periodic table?
The atomic radius generally decreases across a period from left to right.
Compare the ionization energy of metals and noble gases.
Metals have low ionization energy while noble gases have high ionization energy.
Describe how electronegativity changes across the periodic table.
Electronegativity ncreases from left to right across a period and decreases down a group.
How does the metallic character change as you move from left to right across a period on the periodic table?
Metallic character decreases from left to right across a period.
In which group of the periodic table would you expect elements to have similar chemical properties?
Elements in the same group have similar chemical properties.
Why does the atomic radius generally decrease as you move from left to right across a period?
The increase in effective nuclear charge attracts electrons more strongly, leading to a smaller atomic radius.
Explain the factors that influence ionization energy.
Ionization energy increases across a period due to decreasing atomic radius.
Define electronegativity.
Electronegativity is the ability of an atom to attract electrons in a chemical bond.
Compare the metallic character of Group 2 and Group 17.
Group 2 are highly metallic, while Group 17 are nonmetals.
What are the common characteristics of elements in Group 17 and how do they exhibit trends within the group?
Group 17 share characteristics such as high electronegativity and reactivity. Trends within the group show an increase in atomic size and a decrease in electronegativity from top to bottom.
Provide an example of an element that is different from the general trend in atomic radius.
An example would be Helium or Beryllium.
Predict the ionization energy of elements in Group 2 compared to Group 17.
Group 2 has lower ionization energy compared to Group 17.
How does electronegativity influence the type of bond formed between two atoms?
Higher electronegativity leads to the formation of polar covalent or ionic bonds, while lower electronegativity results in nonpolar covalent bonds.
Explain why the metallic character increases down a group on the periodic table.
Down a group, atomic size increases, outer electrons are farther from the nucleus, and electron shielding is more effective, making a more metallic character.
Why do elements in the same group have similar chemical properties?
Because they have the same number of valence electrons and exhibit similar outer electron configurations.