Introductory Inorganic Chemistry CHM 101 Quiz

<p>Placement of noble gases (A)</p> Signup and view all the answers

<p>It limits the number of discovered elements (A)</p> Signup and view all the answers

<p>To understand the periodic classification of elements (B)</p> Signup and view all the answers

<p>The objectives are specific to the principles of introductory inorganic chemistry. (C)</p> Signup and view all the answers

<p>Hydrogen and its compounds (D)</p> Signup and view all the answers

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

<p>Their physical and chemical properties (A)</p> Signup and view all the answers

<p>It explains the arrangement of electrons in atoms. (A)</p> Signup and view all the answers

<p>Fundamental concepts of introductory inorganic chemistry (B)</p> Signup and view all the answers

<p>Biochemical pathways of metabolism (C)</p> Signup and view all the answers

<p>To systematize and organize the elements based on their properties (C)</p> Signup and view all the answers

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

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

<p>Establishing the periodic law (B)</p> Signup and view all the answers

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

<p>Group 2 (D)</p> Signup and view all the answers

<p>Similarities in electron configuration (C)</p> Signup and view all the answers

<p>Create a systematic overview of elemental properties (B)</p> Signup and view all the answers

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

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

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

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

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

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

<p>26 (B)</p> Signup and view all the answers

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

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

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

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

<p>It is smaller by approximately 0.97 (C)</p> Signup and view all the answers

<p>Metallic radii are generally larger (A)</p> Signup and view all the answers

<p>The distance from the nucleus to the edge of the electron cloud (A)</p> Signup and view all the answers

<p>From distances measured between centers of nearest neighbors (B)</p> Signup and view all the answers

<p>They cannot be measured absolutely and are approximated (B)</p> Signup and view all the answers

<p>Metallic bonds have an average bond order less than one (A)</p> Signup and view all the answers

<p>X-ray crystallography (D)</p> Signup and view all the answers

<p>Classification based on the atomic number of elements. (C)</p> Signup and view all the answers

<p>J.N Dobereiner, Dmitri Mendeleev, John Newlands. (D)</p> Signup and view all the answers

<p>A systematic approach to naming elements with atomic number greater than 100. (B)</p> Signup and view all the answers

<p>It uses atomic number instead of atomic mass for arrangement. (A)</p> Signup and view all the answers

<p>To solve disputes between discoverers of the same element. (C)</p> Signup and view all the answers

<p>K is placed before Ar. (D)</p> Signup and view all the answers

<p>The properties of elements recur periodically with increasing atomic number. (A)</p> Signup and view all the answers

<p>Some elements did not fit well into sequence by atomic mass. (C)</p> Signup and view all the answers

The way elements are arranged in a table based on their properties, like atomic number and electron configuration.

The theory that explains the arrangement of elements in the periodic table, stating that elements with similar properties recur periodically.

The distribution of electrons in the different energy levels of an atom. It explains how elements are arranged in the periodic table.

A measure of the size of an atom, essentially the distance from the nucleus to the outermost electron.

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

The tendency of an atom to gain an electron, measured as the energy change when an electron is added to a neutral atom in its gaseous state.

The measure of an atom's ability to attract shared electrons in a chemical bond.

A highly reactive element that forms compounds with all elements except the noble gases. It exists as a diatomic molecule (H2) under standard conditions.

The arrangement of elements in a table based on their properties, like atomic number and electron configuration.

The modern periodic law states that the chemical properties of elements are periodic functions of their atomic numbers. This means that elements with similar properties appear at regular intervals in the periodic table.

The long form of the periodic table is a more detailed and accurate representation of the elements, arranged according to their electronic configurations and grouping them into four blocks: s, p, d, and f.

For elements with atomic numbers greater than 100, the IUPAC (International Union of Pure and Applied Chemistry) has established a specific naming convention based on their atomic numbers and Latin or Greek roots.

The position of elements like potassium (K) and argon (Ar), cobalt (Co) and nickel (Ni), and tellurium (Te) and iodine (I) in the periodic table is determined by their electronic configurations, not just their atomic masses.

The atomic number, representing the number of protons in an atom's nucleus, is the fundamental basis for the periodic classification of elements. Elements with similar atomic numbers share common chemical properties.

The periodic law helps us understand the recurring patterns in the properties of elements. It allows us to predict the characteristics of elements even if they haven't been discovered yet.

Mendeleev's initial periodic table faced limitations, including the inability to incorporate lanthanides and actinides, and the placement of elements with higher atomic weights before those with lower atomic weights, such as Co before Ni and Te before I. He also couldn't accurately predict noble gases or position hydrogen.

The discovery of atomic numbers by Henry Moseley in 1913 led to a crucial revision of Mendeleev's periodic law. Moseley proposed that atomic number, rather than atomic weight, is the fundamental property defining an element's position.

Arranging elements by increasing atomic number resolves many inconsistencies present in Mendeleev's table. The positions of elements like K and Ar, Co and Ni, Te and I are no longer anomalous because arrangement is based on atomic number, not atomic weight.

Isotopes of an element, having the same atomic number, occupy the same position in the periodic table. This highlights the importance of atomic number over atomic weight in determining the arrangement of elements.

The distance between the nucleus of an anion and the point where the nucleus's influence on the electron cloud ends.

The number of nearest neighbors an atom has in a crystal lattice.

A crystal structure where atoms are arranged at the corners and center of a cube.

The distance between the centers of two adjacent ions in a crystal lattice, represents the sum of ionic radii.

Metallic radii are generally larger than the corresponding covalent radii due to weaker and longer metal-metal bonds.

The strength of metallic crystal lattices is attributed to the large number of relatively weaker individual metal-metal bonds.

Values for ionic radii are estimated, not absolutely measured.

X-ray crystallography allows very accurate measurement of the interatomic distance between different ions.

The horizontal rows in the periodic table, numbered 1 to 7. Elements within a period share the same number of electron shells.

The vertical columns in the periodic table, numbered 1 to 18. Elements within a group share similar chemical properties due to having the same number of valence electrons.

A general term for the elements in the first two columns (Groups 1 and 2) and the last six columns (Groups 13 to 18) of the periodic table. They are considered the main part of the table.

These are elements that are located in the two rows below the main body of the periodic table. They have a unique set of properties related to filled f orbitals, and are often called the 'rare earth elements' or the 'inner transition elements.'

A system for organizing elements based on their atomic number and electron configurations, where elements with similar properties recur periodically.

Elements in Periods 6 and 7. These are elements that have their outermost electrons in the f orbital. They are usually characterized by complex color and magnetic properties.

The elements in Group 1 of the periodic table. They are highly reactive metals with a single valence electron, making them eager to react with nonmetals.

The elements in Group 2 of the periodic table. They are reactive metals with two valence electrons that readily form bonds with nonmetals, especially halogens.

The elements in Group 17 of the periodic table. They are highly reactive nonmetals with seven valence electrons that readily gain an electron to form negative ions. They are also known as 'halogens.'

The elements in Group 18 of the periodic table. They are nonreactive gases with a full outer shell of electrons, making them stable and unreactive. They are also known as 'inert gasses.'