Periodic Table Quiz

<p>Halogens (B)</p> Signup and view all the answers

<p>Helium (B)</p> Signup and view all the answers

<p>Along the zigzag line (D)</p> Signup and view all the answers

<p>It is a noble gas (C)</p> Signup and view all the answers

<p>They have the same number of valence electrons (D)</p> Signup and view all the answers

<p>It becomes a positively charged ion. (A)</p> Signup and view all the answers

<p>Recurrence of similar electronic configuration (B)</p> Signup and view all the answers

<p>It increases successively (B)</p> Signup and view all the answers

<p>It decreases down the group. (A)</p> Signup and view all the answers

<p>Valency (A)</p> Signup and view all the answers

<p>Lithium (B)</p> Signup and view all the answers

<p>1 (C)</p> Signup and view all the answers

<p>They are shiny and soft metals. (C)</p> Signup and view all the answers

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

<p>It remains the same (A)</p> Signup and view all the answers

<p>Group 3 to 12 (B)</p> Signup and view all the answers

<p>Negative ion (B)</p> Signup and view all the answers

<p>Halogens (Group 17) (D)</p> Signup and view all the answers

<p>It decreases after Group 14 (A)</p> Signup and view all the answers

<p>7 (C)</p> Signup and view all the answers

<p>It increases down the group. (D)</p> Signup and view all the answers

<p>Combining capacity of an atom (B)</p> Signup and view all the answers

<p>Cl (B)</p> Signup and view all the answers

<p>The atomic size increases down the group. (B)</p> Signup and view all the answers

<p>Period 1 (A)</p> Signup and view all the answers

<p>Group 14 (B)</p> Signup and view all the answers

<p>Group 18 (C)</p> Signup and view all the answers

<p>They have 4 shells. (C), They have the atomic numbers from 19 to 36. (D)</p> Signup and view all the answers

<p>Elements in Group IIIB of the 6th period (D)</p> Signup and view all the answers

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

<p>They are metallic in nature. (A)</p> Signup and view all the answers

<p>lower (B)</p> Signup and view all the answers

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

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

<p>decreases (A)</p> Signup and view all the answers

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

<p>Period 2 (B)</p> Signup and view all the answers

<p>Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine, Neon (D)</p> Signup and view all the answers

<p>Both end with a full outer shell (B)</p> Signup and view all the answers

<p>Non-metallic (B)</p> Signup and view all the answers

<p>Sodium (D)</p> Signup and view all the answers

<p>Increasing non-metallic character (C)</p> Signup and view all the answers

<p>Strontium (A)</p> Signup and view all the answers

<p>Chlorine is smaller than argon (C)</p> Signup and view all the answers

<p>Fluorine (A)</p> Signup and view all the answers

Elements in a single row of the periodic table, sharing the same number of electron shells.

Elements in the same vertical column of the periodic table, sharing the same number of valence electrons.

Elements in Group 1 of the periodic table, except hydrogen, are called alkali metals. These metals are highly reactive and have one valence electron.

Elements in Group 2 of the periodic table are called alkaline earth metals. They are also quite reactive and possess two valence electrons.

Transition elements are located in Groups 3 to 12 of the periodic table. They exhibit a wide range of properties and are often used in various technological applications due to their ability to form colored compounds and act as catalysts.

Elements in Group 17 of the periodic table are called halogens. They are highly reactive non-metals and have seven valence electrons. They form salts when reacting with metals.

Elements in Group 18 of the periodic table are called noble gases. They are unreactive due to their full outer electron shells (eight valence electrons), making them stable and inert.

A property that reappears at regular intervals across the periodic table showing a gradual change (increasing or decreasing) as we move across a period or down a group.

The periodic repetition of similar chemical properties of elements when arranged in increasing order of their atomic numbers.

The repeating patterns of chemical and physical properties of elements when arranged in increasing atomic number.

The number of electron shells an atom has, which determines its position in the periodic table.

The ability of an atom to form chemical bonds by gaining, losing, or sharing electrons.

The number of electrons in the outermost shell of an atom.

The outermost shell of an atom.

In a period, the number of electrons in the valence shell increases from left to right, but valency increases only upto Group 14 and then decreases.

In a group, the number of electrons in the valence shell and therefore the valency, remains the same.

The rows in the periodic table that run left to right.

The columns in the periodic table that run from top to bottom.

The arrangement of electrons in the different shells of an atom.

Across a period, the number of electron shells remains the same, but the number of electrons in the outermost shell increases. This leads to a change in the chemical properties of elements.

As you move down a group, an additional electron shell is added, contributing to the increase in atomic size and affecting chemical behavior.

The tendency of elements with similar electronic configurations to exhibit similar chemical properties.

The outermost shell of an atom.

The number of electrons in the valence shell that are involved in chemical bonding.

Alkali metals belong to Group 1 of the Periodic Table, they are highly reactive and have one valence electron.

Halogens, found in Group 17 of the Periodic Table, are highly reactive non-metals with seven valence electrons.

Elements within the same period have the same number of electron shells but differ in their number of valence electrons.

Elements within the same group have the same number of valence electrons and similar chemical properties due to their comparable electronic configurations.

Increasing electronegativity from left to right, nonmetallic character increases, atomic size decreases, and ionization potential increases across a period.

The electronegativity of elements decreases down a group, while the atomic size increases.

Metals have low ionization potentials and are good reducing agents because they readily lose electrons to form positive ions (cations) while non-metals readily gain electrons to form negative ions (anions).

Electronegativity increases from left to right across a period due to increasing nuclear charge and a decrease in atomic size.

The tendency of an atom in a molecule to attract the shared pair of electrons towards itself.

The number of electron shells an atom has determines its position in a period.

The number of valence electrons (outermost shell electrons) determines an element's group.

The size of an atom's outermost electron shell.

The energy required to remove an electron from a neutral atom in its gaseous state.

The characteristic of being easily oxidized, losing an electron, usually found on the left side of the periodic table.

The characteristic of gaining electrons, usually found on the right side of the periodic table.

The minimum energy required to remove an electron from a gaseous atom in its ground state, forming a positively charged ion.

The energy change when an electron is added to a neutral gaseous atom in its ground state to form a negative ion.

As you move down a group of alkali metals, the atomic size increases. This happens because the number of electron shells increases, making the outermost electron further from the nucleus, leading to weaker attraction and a lower ionisation energy.

As you move down a group of halogens, the atomic size increases. The outermost electron is further from the nucleus, making it more difficult to 'remove' (ionize), so the ionization energy increases.

Alkali metals have low electron affinity because they readily lose their outermost electron, making it less likely to gain another electron.

Halogens have a high electron affinity because they readily gain an electron to complete their outer shell, achieving a stable configuration similar to noble gases.