Which of the following pairs show reverse properties on moving along a period from left to right and from top to down in a group?

The change in enthalpy $[\Delta H]$ in $kJ\ mol^{-1}$ for the reaction is $Mg + 2F \rightarrow MgF_2$. Given: $EA$ of $F = 328\ kJ\ mol^{-1}$, $IE_1$ of $Mg = 737\ kJ\ mol^{-1}$, $IE_2$ of $Mg = 1451\ kJ\ mol^{-1}$.

The ground state electronic configurations of the elements,$U, V, W, X,$ and $Y$ (these symbols do not have any chemical significance) are as follows:
$U: 1s^2 2s^2 2p^3$
$V: 1s^2 2s^2 2p^6 3s^1$
$W: 1s^2 2s^2 2p^6 3s^2 3p^2$
$X: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^2$
$Y: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6$
Determine which sequence of elements satisfies the following statements:
$(i)$ Element forms a carbonate which is not decomposed by heating
$(ii)$ Element is most likely to form coloured ionic compounds
$(iii)$ Element has the largest atomic radius
$(iv)$ Element forms only acidic oxide

Consider the following statements:
$I.$ The radius of an anion is larger than that of the parent atom.
$II.$ The ionization energy generally increases with increasing atomic number in a period.
$III.$ The electronegativity of an element is the tendency of an isolated atom to attract an electron.
Which of the above statements is/are correct?

What are the properties associated with individual particles of matter?

Describe the periodicity of the first ionization enthalpy for elements with atomic numbers $1$ to $60$.