Chemistry Chapter 12 - Chemical Bonding

<p>They form crystalline structures at room temperature (B)</p> Signup and view all the answers

<p>They can exist in any state of matter (solid, liquid, or gas) at room temperature (B)</p> Signup and view all the answers

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

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

<p>Covalent bonds are generally stronger than ionic bonds (C)</p> Signup and view all the answers

<p>Ionic bonds involve transferring electrons to achieve the same amount of electrons as the nearest noble gas, while covalent bonds share to achieve the same amount of electrons as the nearest noble gas. (A)</p> Signup and view all the answers

<p>The bond is formed by the unequal sharing of electrons. (C)</p> Signup and view all the answers

<p>By losing electrons to become a cation. (D)</p> Signup and view all the answers

<p>A compound. (C)</p> Signup and view all the answers

<p>Molecular (covalent) compound. (A)</p> Signup and view all the answers

<p>They are the forces holding atoms together to form a compound or function as a unit. (B)</p> Signup and view all the answers

<p>They lose electrons to form cations. (A)</p> Signup and view all the answers

<p>The configuration of the previous noble gas. (B)</p> Signup and view all the answers

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

<p>The difference in electronegativity between the elements in sodium fluoride is larger. (D)</p> Signup and view all the answers

<p>Molecular polarity is a consequence of dipole moment. (A)</p> Signup and view all the answers

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

<p>As ∆EN increases, the bond becomes more polar. (B)</p> Signup and view all the answers

<p>Water is a polar solvent, and ionic compounds have a polar structure. (C)</p> Signup and view all the answers

<p>The difference in electronegativity between the atoms (B)</p> Signup and view all the answers

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

<p>Metals usually lose electrons to form cations. (D)</p> Signup and view all the answers

<p>4.0 (A)</p> Signup and view all the answers

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

<p>Unequal sharing of electrons resulting in charge separation. (D)</p> Signup and view all the answers

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

<p>Non-metals generally attract electrons better due to higher electronegativity. (A)</p> Signup and view all the answers

<p>It increases, leading to higher electronegativity. (D)</p> Signup and view all the answers

<p>-78 °C (B)</p> Signup and view all the answers

<p>Pure ionic bond (A)</p> Signup and view all the answers

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

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

<p>Strong polar covalent bond (A)</p> Signup and view all the answers

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

<p>The difference in electronegativity (∆EN) (D)</p> Signup and view all the answers

<p>1.9 (D)</p> Signup and view all the answers

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

<p>The bond's polarity and ionic character (D)</p> Signup and view all the answers

<p>Electrons are shared equally, resulting in a pure covalent bond (D)</p> Signup and view all the answers

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

<p>The bond becomes more polar (D)</p> Signup and view all the answers

<p>Charge separation within a molecule (C)</p> Signup and view all the answers

<p>Electronegativity increases across a period and decreases down a group (C)</p> Signup and view all the answers

<p>In bonds between nonmetals and metals with a moderate electronegativity difference (A)</p> Signup and view all the answers

<p>The negative charge center (D)</p> Signup and view all the answers

A chemical combination of two or more elements. Metal and non-metal elements form ionic compounds. Non-metal and non-metal elements form molecular compounds (also called covalent compounds).

The forces that hold groups of atoms together to form a compound or function as a unit. Atoms are bonded in two ways: by transferring electrons from one atom to another (ionic bond) or by sharing electrons among the participating atoms (covalent bond).

A stable bond is formed when participating atoms achieve a noble gas electron configuration, having the same number of electrons as a noble gas atom (e.g., He (2 electrons), Ne (10 electrons), Ar (18 electrons).

Metals lose one or more outermost electrons to achieve the previous noble gas configuration, forming positively charged ions called cations.

Non-metals gain electrons to achieve the next noble gas configuration, forming negatively charged ions called anions.

Atoms share electrons to achieve a stable noble gas electron configuration.

The tendency of an atom in a molecule to attract shared electrons toward itself. Higher electronegative (EN) atoms attract electrons more strongly.

A covalent bond where electrons are shared unequally between atoms due to differences in electronegativity, creating partial positive and negative charges within the molecule.

Nonmetal atoms achieve a stable electron configuration by gaining one or more electrons to become negatively charged ions called anions.

Nonmetal atoms share electrons to achieve a stable electron configuration, forming a covalent bond.

A series of ions or atoms possessing the same number of electrons.

A compound formed from the electrostatic attraction between oppositely charged ions, typically a metal and a nonmetal.

A compound formed when nonmetal atoms share electrons, resulting in molecules.

Ionic compounds typically exhibit high melting points due to the strong electrostatic attraction between ions.

Ionic compounds are good conductors of electricity when dissolved in water or melted because the ions are free to move and carry charge.

Molecular compounds typically have lower melting points compared to ionic compounds because the weaker intermolecular forces are easier to overcome.

The difference in electronegativity between two atoms in a bond.

Electronegativity increases across a period from left to right (excluding noble gases).

Electronegativity decreases down a group.

Non-metals generally have higher electronegativity than metals.

The rule that states that atoms tend to gain, lose, or share electrons to achieve eight valence electrons (like a noble gas).

A bond between atoms where electrons are shared equally.

A bond where electrons are completely transferred from one atom to another, forming ions.

The difference in electronegativity between two atoms in a bond.

A chemical bond with a greater degree of electron sharing.

A chemical bond with a greater degree of electron transfer.

Substances with similar ionic character tend to dissolve in each other.

A measure of electron distribution in a molecule, represented by a vector pointing from the partial positive charge to the partial negative charge.

The difference in electronegativity between two bonded atoms determines the polarity of a bond.

A molecule with a dipole moment due to unequal charge distribution, creating a positive and negative end.

A molecule with no dipole moment due to evenly distributed charge.

The overall attraction between molecules, which depends on dipole moments.

The difference in electronegativity between two atoms bonded together.

A bond with a smaller electronegativity difference than an ionic bond, indicating a partial transfer of electrons and both ionic and covalent character.