I can tell you there certainly is enough information, so we can eliminate the fourth option right away.
Group two elements tend to form 2+ cations, and nitrogen forms 3- anions. To make a stable substance, we need those to cancel out. Calling the group 2 element X:
N2X3 would cause the charge to be 2(-3) + 3(2) = 0
This would mean 3 ions of X and 2 anions of N would be a stable ionic compound.
The atomic weight of the naturally occurring element would
simply be the weighted average of the two isotopes. Calculating:
atomic weight = (25.2 g / mol) * 0.801 + (29.4 g / mol) *
(1 – 0.801)
<span>atomic weight = 26.04 g / mol</span>
<u>Answer:</u>
<em>A solution that has fewer neutrons than protons and more electrons than protons is a negative ion.
</em>
<u>Explanation:</u>
<em>Atoms in their original state have equal number of protons and electrons. The subatomic particles that take part in reaction are electrons.</em> When the electrons of an atom involve in a reaction an atom may lose or gain electrons and reach ionic state.
Ions can be positively charged or negatively charged and the charge acquired depends on whether electrons are gained or lost. The process of <em>losing electrons make an atom a positively charged ion and gaining electrons make an atom a negatively charged ion. </em>
<em>In this case the number of electrons is more than the number of protons which means there is an excess of negative charge and the atom has become a negatively charged ion.
</em>
(Missing in the question) solubility in g per 100 mL of water:
CdI2 86.2 (cold water) so,
-We will heat a saturation solution of CdI2 [86.2 g / 100 mL], by the effect of the heat the solution will be unsaturated and dissolve more CdI2 when reaching a high temperature. and let the solution cools again by itself and covers it well to make sure there is no dust in it. when it reaches back to the cold water temperature, we will find the solution is supersaturated and all the solute will stay dissolved.
The density of a substance is its mass per unit volume, given by the mass divided by the volume. Density depends on the substance of concern and doesn't matter whether one has a little amount of it or a whole full of it. Therefore, the density of the two smaller pieces is now the same as the original density.
