Periodic Table Overview and History

<p>Two different elements occupied the same cell. (A)</p> Signup and view all the answers

<p>Every eighth element shares similar chemical properties. (A)</p> Signup and view all the answers

<p>Dmitri Mendeleev and Lothar Meyer (D)</p> Signup and view all the answers

<p>Atomic properties of elements reflect a pattern based on increasing atomic masses. (C)</p> Signup and view all the answers

<p>Density at room temperature (C)</p> Signup and view all the answers

<p>The atomic radius increases due to increased energy levels. (D)</p> Signup and view all the answers

<p>Elements in the same group share similar properties due to similar valence electron configurations. (B)</p> Signup and view all the answers

<p>Group 8A (B)</p> Signup and view all the answers

<p>d-block (B)</p> Signup and view all the answers

<p>It increases due to increased nuclear charge. (C)</p> Signup and view all the answers

<p>Electronegativity (C)</p> Signup and view all the answers

<p>Alkali Metals (Group 1A) (A)</p> Signup and view all the answers

<p>Increased number of protons results in greater nuclear attraction. (C)</p> Signup and view all the answers

<p>Removal of an electron from a p-orbital instead of an s-orbital (B)</p> Signup and view all the answers

<p>More negative values of electron affinity indicate higher attraction for electrons. (C)</p> Signup and view all the answers

<p>Repulsion from s-electrons when the added electron goes into a p-orbital (B)</p> Signup and view all the answers

<p>Decreases from top to bottom and increases from left to right (B)</p> Signup and view all the answers

<p>Increased distance of electrons from the nucleus (A)</p> Signup and view all the answers

A table that arranges all known elements in rows and columns based on their atomic properties.

Elements arranged by increasing atomic mass show repeating patterns of properties.

The first modern periodic table, predicting undiscovered elements.

Elements arranged by increasing atomic number show repeating patterns of properties.

The middle element in a triad has properties roughly the average of the other two.

Elements with similar properties repeat every 8 elements when arranged by increasing atomic weight.

The number of protons in an atom's nucleus, used in modern periodic table organization.

Recurring patterns in elements' properties across the periodic table.

Ionization energy slightly decreases between Groups IIA and IIIA, due to electrons being removed from a p-orbital (further from the nucleus) rather than an s-orbital.

Ionization energy slightly increases between Groups VA and VIA because the electron removed is from a doubly occupied orbital, experiencing repulsion from the other electron.

Electron affinity decreases as you move down a group in the periodic table. Atoms become larger, and the added electron is farther from the nucleus, resulting in weaker attraction.

Electron affinity generally increases as you move across a period. Atoms become smaller, making the added electron closer to the nucleus and experiencing stronger attraction.

Electron affinity decreases between Groups IA and IIA because the added electron enters a p-orbital, further from the nucleus and experiencing repulsion from s-electrons.

Vertical columns in the periodic table, representing groups or families of elements with similar chemical properties.

Horizontal rows in the periodic table, representing the energy level of the elements' outermost electrons, contributing to periodic trends.

Elements in groups 1A to 8A (excluding transition metals) exhibiting a wide range of properties and reactivity.

Elements in groups 3B to 12B (excluding lanthanides and actinides) known for their variable oxidation states and complex compounds.

Elements in groups 1A (alkali metals) and 2A (alkaline earth metals), characterized by their outermost electron residing in the 's' orbital.

Elements in groups 3A to 8A, characterized by their outermost electron residing in the 'p' orbital, with a wide range of properties and reactivity.

Elements in groups 3B to 12B, characterized by their outermost electron residing in the 'd' orbital, exhibiting metallic properties and diverse oxidation states.

Elements in the two rows below the main periodic table (lanthanides and actinides), characterized by their outermost electron residing in the 'f' orbital.