periodic table trends
electronegativity and ionization energy trend.
9. define each of the trends
a. electronegativity
b. ionization energy
the image below is a chart that shows these two periodic trends of elements. ignore the other trends in the image.

10. explain how ionization energy changes moving from left to right across a period.
11. explain how ionization energy changes moving down a group.
12. explain how electronegativity changes moving from left to right across a period.
13. explain how electronegativity changes moving down a group.

the image on the right is a chart that shows how
the atomic radius (size of the atom) decreases in
size from left to right in a period and increases
from top to bottom in a group.
14. use an arrow to show the atomic radius trend
along a period and down a group.
15. explain how and why the number of protons
and electrons in the outer shell contributes to
the change in atomic radius

Question

periodic table trends
electronegativity and ionization energy trend.
9. define each of the trends
   a. electronegativity
   b. ionization energy
the image below is a chart that shows these two periodic trends of elements. ignore the other trends in the image.

10. explain how ionization energy changes moving from left to right across a period.
11. explain how ionization energy changes moving down a group.
12. explain how electronegativity changes moving from left to right across a period.
13. explain how electronegativity changes moving down a group.

the image on the right is a chart that shows how
the atomic radius (size of the atom) decreases in
size from left to right in a period and increases
from top to bottom in a group.
14. use an arrow to show the atomic radius trend
    along a period and down a group.
15. explain how and why the number of protons
    and electrons in the outer shell contributes to
    the change in atomic radius

Accepted Answer

### For question 9a (Define Electronegativity):
# Brief Explanations:
Electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself when forming a chemical bond. It helps in predicting bond polarity, molecular polarity, and the nature of chemical interactions between atoms.
# Answer:
Electronegativity is the tendency of an atom to attract bonded electrons towards itself.

### For question 9b (Define Ionization Energy):
# Brief Explanations:
Ionization energy is the minimum amount of energy required to remove the most loosely bound electron (the valence electron) from an isolated gaseous atom or ion in its ground state. It is an indicator of the ease or difficulty with which an atom loses an electron, and it shows trends across periods (increases) and down groups (decreases) in the periodic table.
# Answer:
Ionization energy is the energy needed to remove a valence electron from a gaseous atom/ion.

### For question 10 (Ionization Energy across a Period - Left to Right):
# Brief Explanations:
As we move from left to right across a period in the periodic table, the ionization energy generally increases. This is because the atomic number (number of protons) increases, leading to a greater nuclear charge. The electrons are added to the same valence shell (since we are in the same period), so the electron shielding effect from inner shells remains relatively constant. The increased nuclear charge pulls the valence electrons more strongly towards the nucleus, making it harder to remove an electron (thus requiring more energy, i.e., higher ionization energy).
# Answer:
Ionization energy increases left - to - right across a period due to increasing nuclear charge (same valence shell, constant shielding), making electron removal harder.

### For question 11 (Ionization Energy down a Group):
# Brief Explanations:
When moving down a group in the periodic table, the ionization energy generally decreases. This is because as we go down a group, the number of electron shells (energy levels) increases. The valence electrons are located in shells that are further from the nucleus. Although the nuclear charge also increases, the increase in the number of inner electron shells leads to a significant increase in electron shielding. The valence electrons experience a much weaker effective nuclear charge (due to shielding), so they are held less tightly and are easier to remove, resulting in lower ionization energy.
# Answer:
Ionization energy decreases down a group as electron shells increase (more shielding), weakening the hold on valence electrons.

### For question 12 (Electronegativity across a Period - Left to Right):
# Brief Explanations:
Electronegativity generally increases as we move from left to right across a period. The reason is similar to the ionization energy trend across a period: the nuclear charge increases while the electrons are added to the same valence shell, and shielding remains relatively constant. A higher nuclear charge means the atom has a stronger ability to attract the shared electrons in a chemical bond, so electronegativity increases.
# Answer:
Electronegativity increases left - to - right across a period due to increasing nuclear charge (same shell, constant shielding) for stronger electron attraction.

### For question 13 (Electronegativity down a Group):
# Brief Explanations:
Electronegativity generally decreases as we move down a group. This is because, as we go down a group, the number of electron shells increases. The valence electrons are further from the nucleus, and there is more electron shielding from the inner shells. The effective nuclear charge experienced by the valence electrons is reduced, so the atom's ability to attract shared electrons in a bond (electronegativity) decreases.
# Answer:
Electronegativity decreases down a group as electron shells increase (more shielding), reducing the effective nuclear charge on valence electrons.

### For question 14 (Atomic Radius Trend - Arrow Representation):
# Brief Explanations:
- **Across a Period (Left to Right)**: The atomic radius decreases. So, we draw an arrow from the left - most element of a period to the right - most element, pointing to the right (to show the decrease in size). For example, in period 2, from Li to Ne, the arrow would go from Li towards Ne, indicating a decrease in atomic radius.
- **Down a Group (Top to Bottom)**: The atomic radius increases. So, we draw an arrow from the top element of a group to the bottom element, pointing downwards (to show the increase in size). For example, in group 1, from H to Fr, the arrow would go from H towards Fr, indicating an increase in atomic radius.
# Answer:
- Across a period: Arrow from left to right (decreasing radius).
- Down a group: Arrow from top to bottom (increasing radius).

### For question 15 (Protons, Electrons, and Atomic Radius):
# Brief Explanations:
- **Across a Period (Left to Right)**:
    - The number of protons in the nucleus increases (due to increasing atomic number). This leads to a greater nuclear charge.
    - The number of electrons in the outer shell also increases, but they are added to the same valence shell (since we are in the same period).
    - The increase in nuclear charge pulls the outer - shell electrons more strongly towards the nucleus. Even though the number of outer - shell electrons increases, the shielding from inner electrons remains relatively constant. So, the electrons are pulled closer to the nucleus, resulting in a decrease in atomic radius.
- **Down a Group (Top to Bottom)**:
    - The number of protons increases, but the number of electron shells (energy levels) also increases.
    - The outer - shell electrons are in shells that are further from the nucleus.
    - The increase in the number of inner electron shells leads to a significant increase in electron shielding. The effective nuclear charge experienced by the outer - shell electrons is reduced (because the inner electrons shield the outer electrons from the full nuclear charge). So, the outer - shell electrons are held less tightly and are further from the nucleus, leading to an increase in atomic radius.
# Answer:
- Across a period: Increasing protons (same shell, constant shielding) pull outer electrons closer, decreasing radius.
- Down a group: More shells (more shielding) weaken the hold on outer electrons, increasing radius.

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

For question 9a (Define Electronegativity):

Answer:

For question 9b (Define Ionization Energy):