Question

part a. what is the definition of reactivity?
part b. what is the trend in the reactivity of metals as you go across the periodic table from left to right?
part c. what is the trend in the reactivity of metals as you go down the periodic table from top to bottom?
part d. what is the trend in the reactivity of nonmetals as you go across the periodic table from left to right?
part e. what is the trend in the reactivity of nonmetals as you go down the periodic table from top to bottom?

Explanation:

Part A:

Reactivity is the tendency of an element to undergo a chemical reaction, either by losing, gaining, or sharing electrons, often to achieve a stable electron configuration (like a noble gas configuration). It relates to how easily an element forms compounds or participates in reactions.

Part B:

As you move from left to right across a period (row) in the periodic table for metals, reactivity generally decreases. This is because metals tend to lose electrons. As you go right, atomic radius decreases (nuclear charge increases, pulling electrons closer), so it’s harder for metals to lose electrons (ionization energy increases), making them less reactive. For example, alkali metals (left) are very reactive, while transition metals (middle-right) are less reactive.

Part C:

As you go down a group (column) for metals, reactivity generally increases. This is because atomic radius increases (electrons are in higher energy levels, farther from the nucleus), so it’s easier for metals to lose electrons (ionization energy decreases). For example, lithium (top of Group 1) is less reactive than sodium or potassium (below it) because the outer electron in lower periods is more easily removed.

Part D:

For nonmetals, as you move from left to right across a period, reactivity generally increases. Nonmetals tend to gain electrons. As you go right, atomic radius decreases (nuclear charge increases), so the nucleus attracts electrons more strongly (electronegativity increases), making nonmetals more reactive (e.g., fluorine, on the far right, is extremely reactive as a nonmetal).

Part E:

For nonmetals, as you go down a group, reactivity generally decreases. Atomic radius increases (electrons are farther from the nucleus), so the nucleus has less attraction for additional electrons (electronegativity decreases). For example, fluorine (top of Group 17) is more reactive than chlorine, bromine, or iodine (below it) because it can attract electrons more easily.

Answer:

Part A:

Reactivity is an element’s tendency to undergo chemical reactions (lose/gain/share electrons) to achieve stability (e.g., noble gas electron configuration).

Part B:

Metals’ reactivity decreases from left to right across a period.

Part C:

Metals’ reactivity increases from top to bottom in a group.

Part D:

Nonmetals’ reactivity increases from left to right across a period.

Part E:

Nonmetals’ reactivity decreases from top to bottom in a group.