Atomic Properties Quiz

Atomic radius decreases across a period from left to right and increases down a group from top to bottom.

Ionization energy increases across a period from left to right and decreases down a group from top to bottom.

Electronegativity is the ability of an atom to attract electrons. It increases across a period from left to right and decreases down a group.

<p>Electron affinity is the energy change that occurs when an electron is added to a gaseous atom. It generally increases down the groups and decreases across a period from left to right.</p> Signup and view all the answers

<p>Cations, formed by the loss of electrons, are smaller than their neutral atoms due to reduced electron-electron repulsion.</p> Signup and view all the answers

<p>The melting and boiling points increase from group I to group IV across periods.</p> Signup and view all the answers

<p>Electropositivity is the ability of an atom to lose electrons and form positive ions. It decreases across a period from left to right and increases down a group.</p> Signup and view all the answers

<p>The valence electron configuration for alkali metals is $ns^1$, where $n$ represents the period number.</p> Signup and view all the answers

<p>The ionic radius of non-metals generally decreases across periods.</p> Signup and view all the answers

<p>The ease of formation of ions for non-metals increases from Group IV to Group VII across periods due to increasing electron affinity.</p> Signup and view all the answers

<p>Lithium and magnesium both form normal oxides and have similar solubility characteristics in water.</p> Signup and view all the answers

<p>Metallic character increases as you move down the groups in the periodic table due to decreasing ionization energy.</p> Signup and view all the answers

<p>The ease of gaining electrons decreases for halogens as you move down the group.</p> Signup and view all the answers

<p>Chemical reactivity of alkaline earth metals increases down the group due to lower ionization energies.</p> Signup and view all the answers

<p>Beryllium and Aluminium both exhibit similar behavior in forming compounds with similar stoichiometries.</p> Signup and view all the answers

<p>Ionization energy increases across periods, making it more difficult for non-metals to lose electrons.</p> Signup and view all the answers

<p>Ionic radius generally decreases across a period due to increasing nuclear charge, which pulls electrons closer to the nucleus.</p> Signup and view all the answers

<p>Melting points generally increase from Group I to Group III due to stronger metallic bonds and a transition to giant covalent structures.</p> Signup and view all the answers

<p>Chemical reactivity for non-metals increases from Group IV to Group VII across the periods.</p> Signup and view all the answers

<p>Electron affinity increases across periods as elements become more electronegative and better at attracting electrons.</p> Signup and view all the answers

<p>Atomic size increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.</p> Signup and view all the answers

<p>Ionization energy generally increases across a period as the atomic radius decreases and nuclear charge increases.</p> Signup and view all the answers

<p>Higher electronegativity in non-metals indicates greater ability to attract electrons, making them more reactive.</p> Signup and view all the answers

<p>Thermal stability of compounds generally decreases from Group I to III for metals and increases from Group IV to VII for non-metals.</p> Signup and view all the answers