Chemical Bonding (Part 1)

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

<p>Group 16 (B)</p> Signup and view all the answers

<p>By adding -ide to the root of the name (B)</p> Signup and view all the answers

<p>-3 (D)</p> Signup and view all the answers

<p>Anions are larger than their original atoms (D)</p> Signup and view all the answers

<p>It involves the electrostatic attraction between oppositely charged ions. (C)</p> Signup and view all the answers

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

<p>Cations are formed when metal atoms lose valence electrons. (A)</p> Signup and view all the answers

<p>Free-moving ions in solution (C)</p> Signup and view all the answers

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

<p>Anions are formed when non-metal atoms gain electrons. (C)</p> Signup and view all the answers

<p>Na2SO4 (C)</p> Signup and view all the answers

<p>The size of the atom decreases. (A)</p> Signup and view all the answers

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

<p>Mg2+ (B)</p> Signup and view all the answers

<p>Ionic compounds have higher melting and boiling points (D)</p> Signup and view all the answers

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

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

<p>The cation (metal) (A)</p> Signup and view all the answers

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

<p>Conduct electricity in solid form (D)</p> Signup and view all the answers

<p>Pb(NO3)2 (D)</p> Signup and view all the answers

<p>Electrons are shared unequally due to electronegativity differences. (C)</p> Signup and view all the answers

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

<p>Energy is released. (C)</p> Signup and view all the answers

<p>By examining the electronegativity differences between the atoms. (C)</p> Signup and view all the answers

<p>A bond between carbon and carbon. (B)</p> Signup and view all the answers

<p>FeCl3 (A)</p> Signup and view all the answers

<p>Non-polar covalent bond (D)</p> Signup and view all the answers

<p>Less than 0.4 (C)</p> Signup and view all the answers

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

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

<p>Soft and flexible nature (B)</p> Signup and view all the answers

<p>The arrangement of valence electrons among atoms (A)</p> Signup and view all the answers

<p>They do not conduct electricity (A)</p> Signup and view all the answers

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

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

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

<p>It increases the count by 1. (C)</p> Signup and view all the answers

<p>5 from nitrogen + 4 from hydrogen - 1 from positive charge (A)</p> Signup and view all the answers

<p>The atom with the lowest electronegativity (D)</p> Signup and view all the answers

<p>Two valence electrons per bond (C)</p> Signup and view all the answers

<p>They are marked on the central atom. (D)</p> Signup and view all the answers

<p>To minimize the formal charge on atoms (D)</p> Signup and view all the answers

<p>One electron is counted for each atom in the bond. (C)</p> Signup and view all the answers

A negatively charged ion formed when a nonmetal gains electrons.

A positively charged ion formed when a metal loses electrons.

A chemical compound formed by the electrostatic attraction between positively charged cations and negatively charged anions.

A regular, repeating arrangement of ions in a solid ionic compound.

The electrostatic attraction between oppositely charged ions in an ionic compound.

A group of atoms that carry a net electrical charge.

The process of writing the chemical formula of an ionic compound by balancing the charges of the cation and anion.

The overall charge on an ion, indicated by a superscript number and a plus or minus sign.

Elements in group 2 of the periodic table form +2 cations.

Elements in group 3 of the periodic table form +3 cations.

Metals in groups other than 1, 2, or 3 form cations with variable charges, making it harder to predict.

Cations formed by single atoms are called monatomic cations.

The names of monatomic cations typically start with the metal name and include a Roman numeral indicating the charge.

The charge of an anion is determined by the number of electrons gained, represented with a minus sign.

Monatomic anions are named by adding the suffix -ide to the root name of the nonmetal.

The number of electrons an atom can gain or lose to achieve a stable electron configuration.

The number of electrons that an atom can gain, lose or share to form a chemical bond.

The process where an atom loses electrons to become positively charged.

The charge on a cation is determined by the number of electrons lost, followed by a '+' symbol.

Predicting the charge of a monatomic cation can be done by looking at its group number on the periodic table, such as alkali metals in group 1 always forming +1 cations.

The tendency of an atom to attract electrons towards itself when it is forming a chemical bond.

A covalent bond where the electrons are shared equally between the atoms.

A covalent bond where the electrons are shared unequally between the atoms.

A molecule or ion formed by two or more atoms that are joined together by covalent bonds.

A type of covalent bonding where the electrons are shared between two atoms.

A covalent structure where the atoms are connected in a continuous network.

A type of covalent bonding where two pairs of electrons are shared between two atoms.

A chemical bond formed by the sharing of one or more pairs of electrons between two atoms.

A force that holds atoms together in a molecule. It arises from the electrostatic attraction between the positively charged nuclei and the negatively charged electrons.

Energy is released when bonds form, and energy is required (absorbed) to break bonds.

A molecule with a separation of electrical charge, resulting in a positive and a negative end.

A molecule with no separation of electrical charge, due to the equal sharing of electrons.

The sum of the valence electrons contributed by each atom in a molecule or ion, considering any charge.

The central atom in a molecule is typically the element with lower electronegativity, except for hydrogen (H).

The most electronegative atom is given priority when distributing remaining valence electrons after forming bonds in a molecule.

In a bond, each atom is assigned one electron. For lone pairs, both electrons are assigned to the atom.

The formal charge is calculated by comparing the number of electrons in the atom's non-bonded state (free atom) to the number of electrons assigned to it in the molecule or ion.

Lone pairs of electrons can be converted into bonding pairs to minimize formal charge and complete octets in molecules.

In a Lewis structure, a shared pair of electrons between two atoms is represented as a single bond.

To satisfy the octet rule, elements in the second row of the periodic table aim to have eight electrons in their valence shell by forming bonds and acquiring lone pairs.