Question

the chemical reactivity of nonmetals generally increases as you move:
from right to left across a period
up a group
from left to right across a period, then down a group
down a group
true or false. polar compounds are attracted to both positive and negative charges.
true
false
what is the primary driving force for the formation of a mg²⁺ ion from a neutral magnesium atom?
to decrease the nuclear charge of magnesium
to achieve a stable octet configuration like neon
to increase the atomic radius of magnesium
to maximize the number of valence electrons

Explanation:

First Question (Chemical Reactivity of Nonmetals)

For nonmetals, across a period (left - right), effective nuclear charge increases, so reactivity (ability to gain electrons) increases. Down a group, atomic size increases but for nonmetals, the trend is more complex, but the general trend of increasing reactivity is left - right across period and then down group (as electronegativity and electron - gaining ability follow this for nonmetals in general). The other options: moving right - left across period decreases reactivity; moving up a group (smaller atoms, but for nonmetals, down group can have increasing reactivity in some cases related to bond - forming, and left - right across period is a key increase); moving down a group alone is not the main general increase trend.

Second Question (Polar Compounds and Charges)

Polar compounds have a partial positive and a partial negative end (dipole). The partial positive end is attracted to negative charges, and the partial negative end is attracted to positive charges. So polar compounds are attracted to both positive and negative charges.

Third Question (Formation of \(Mg^{2+}\) Ion)

A neutral Mg atom has an electron configuration of \(1s^{2}2s^{2}2p^{6}3s^{2}\). When it forms \(Mg^{2+}\), it loses 2 electrons from the 3s orbital, resulting in an electron configuration of \(1s^{2}2s^{2}2p^{6}\), which is the same as the stable noble gas neon (octet configuration). The other options: nuclear charge is determined by protons, can't be changed by ion formation; forming a cation (losing electrons) decreases atomic radius, not increases; and the goal is to achieve a stable electron configuration, not to maximize valence electrons (Mg loses valence electrons to achieve octet, not maximize them).

Answer:

From left to right across a period, then down a group