Question

a) define first ionization energy
b) first ionization energy from left to right.
c) first ionization energy from top to bottom.
d) which of the following atoms has the highest first ionization energy?
mg fr f rb n b

1. electronegativity

a) define electronegativity:
b) electronegativity from left to right.
c) electronegativity from top to bottom.
d) which of the following atoms is the least electronegative?
be ca cl p al ba
e) which of the following atoms is the most electronegative?
o li ne k c cs

Explanation:

• a) First ionization energy is the energy required to remove the outermost electron from a neutral atom in the gas phase.
• b) First ionization energy generally increases from left to right across a period in the periodic table. This is because as we move from left to right, the nuclear charge increases while the shielding effect remains relatively constant, making it more difficult to remove an electron.
• c) First ionization energy generally decreases from top to bottom within a group in the periodic table. As we move down a group, the number of electron shells increases, and the outermost electrons are farther from the nucleus, experiencing less effective nuclear charge and being easier to remove.
• d) Among the given atoms (Mg, Fr, F, Rb, N, B), F (fluorine) has the highest first ionization energy. Fluorine is a small atom with a high nuclear charge and a strong attraction for its electrons.
• 5. a) Electronegativity is the measure of an atom's ability to attract electrons towards itself in a chemical bond.
• 5. b) Electronegativity generally increases from left to right across a period. Similar to ionization energy, the increasing nuclear charge and relatively constant shielding make atoms more electronegative as we move right.
• 5. c) Electronegativity generally decreases from top to bottom within a group. The increased distance of the outermost electrons from the nucleus reduces the atom's ability to attract electrons.
• 5. d) Among the given atoms (Be, Ca, Cl, P, Al, Ba), Ba (barium) is the least electronegative. Barium is a large atom with a relatively low nuclear charge compared to the other atoms, and its electrons are more loosely held.
• 5. e) Among the given atoms (O, Li, Ne, K, C, Cs), O (oxygen) is the most electronegative. Oxygen has a relatively high nuclear charge and a strong tendency to attract electrons in a bond.

Answer:

a) The energy required to remove the outermost electron from a neutral atom in the gas phase.
b) Increases
c) Decreases
d) F

1. a) The measure of an atom's ability to attract electrons towards itself in a chemical bond.
2. b) Increases
3. c) Decreases
4. d) Ba
5. e) O