Chemical Bonds and Ionic Bonds

<p>Hydrofluoric Acid (HF) and Fluoride Ion (F⁻) (D)</p> Signup and view all the answers

<p>Water (H₂O) (C)</p> Signup and view all the answers

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

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

<p>It loses two electrons to become Mg²⁺ (A)</p> Signup and view all the answers

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

<p>Number of electrons (D)</p> Signup and view all the answers

<p>They involve the sharing of electrons between atoms (B)</p> Signup and view all the answers

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

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

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

<p>A bond formed when atoms transfer electrons to each other. (D)</p> Signup and view all the answers

<p>They have a complete valence electron shell. (B)</p> Signup and view all the answers

<p>4 (A)</p> Signup and view all the answers

<p>A diagram representing the arrangement of atoms and electrons in a molecule. (B)</p> Signup and view all the answers

<p>The Octet Rule states that atoms tend to have eight electrons in their outermost shell. (C)</p> Signup and view all the answers

<p>Valency predicts the type of bond an atom will form. (D)</p> Signup and view all the answers

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

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

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

<p>Difference in electronegativity (B)</p> Signup and view all the answers

<p>They include dipole-dipole interactions. (D)</p> Signup and view all the answers

<p>Oxygen (O₂) (C)</p> Signup and view all the answers

<p>Johannes van der Waals (A)</p> Signup and view all the answers

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

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

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

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

<p>Water (H₂O) (D)</p> Signup and view all the answers

<p>It cancels bond dipoles, resulting in nonpolar molecules (A)</p> Signup and view all the answers

<p>It has a polar bond due to electronegativity difference (B)</p> Signup and view all the answers

<p>It has symmetrical shape that cancels bond dipoles (C)</p> Signup and view all the answers

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

<p>Ion-Dipole Forces (A)</p> Signup and view all the answers

<p>Potassium Ion (K⁺) (D)</p> Signup and view all the answers

<p>Dipole-Induced Forces (B)</p> Signup and view all the answers

<p>Hydrofluoric Acid (HF) with other HF molecules (A)</p> Signup and view all the answers

<p>Ethanol's polarity (A)</p> Signup and view all the answers

<p>They are associated with induced dipoles. (C)</p> Signup and view all the answers

<p>When salts dissolve in polar solvents (A)</p> Signup and view all the answers

<p>Attractions between polar molecules (C)</p> Signup and view all the answers

Elements in Group 18 with complete valence shells, stable and unreactive.

Helium (He), Argon (Ar), Xenon (Xe) are noble gases known for their stability.

The combining power of an element, determined by its outermost electron count.

A diagram showing bonding and lone pairs of electrons in a molecule.

Bonds formed when one atom donates electrons, creating oppositely charged ions.

Most atoms strive to have eight electrons in their valence shell to be stable.

Water consists of two hydrogen atoms (1 valence electron each) and one oxygen atom (6 valence electrons).

Carbon dioxide has one carbon (4 valence electrons) and two oxygens (6 valence electrons each).

Ionic compounds form when metals lose electrons and nonmetals gain them, creating charged ions.

NaCl forms when sodium loses one electron to become Na⁺ and chlorine gains one electron to become Cl⁻.

MgO forms when magnesium loses two electrons to become Mg²⁺ and oxygen gains two electrons to become O²⁻.

CaF₂ forms when calcium loses two electrons to become Ca²⁺ and two fluorine gain one electron each to become F⁻.

Covalent bonds form when two nonmetals share electrons to fill their outer shells.

Water forms when oxygen shares electrons with two hydrogen atoms, creating two single bonds.

Methane forms when carbon shares electrons with four hydrogen atoms, resulting in four single bonds.

Carbon dioxide forms when carbon forms double bonds with two oxygen atoms.

A strong type of dipole-dipole interaction between molecules with hydrogen bonded to electronegative atoms.

Acid-base pairs where one donates a proton and the other accepts it, transforming during a reaction.

Weak, temporary attractive forces arising from temporary dipoles in atoms or molecules, present in all substances.

The negative logarithm (base 10) of the hydrogen ion concentration in a solution, indicating acidity or basicity.

Pairs like acetic acid and acetate, where one transforms to the other by donating or accepting a proton.

The property of a bond or molecule that results from a difference in electronegativity between atoms, leading to an uneven distribution of charge.

A measure of an atom’s ability to attract electrons towards itself when forming a chemical bond.

A type of bond where one pair of electrons is shared between two atoms.

A bond in which two pairs of electrons are shared between two atoms.

A bond characterized by three pairs of shared electrons between two atoms.

Determined by the difference in electronegativity between two bonded atoms; a large difference results in a polar bond.

Defined by the polarities of individual bonds and the overall shape of the molecule; symmetrical shapes might cancel out dipoles.

Water (H₂O) is bent, leading to a polar structure; Hydrogen Chloride (HCl) has a significant bond dipole due to electronegativity differences.

A polar molecule with a trigonal pyramidal shape due to lone pair repulsion.

A diatomic polar molecule due to a difference in electronegativity between hydrogen and chlorine.

The three-dimensional arrangement of atoms in a molecule determined by electron pair repulsions.

Attractions between molecules, weaker than intramolecular forces, impacting physical properties.

Strong bonds that hold atoms together within a molecule, such as ionic and covalent bonds.

Forces of attraction between polar molecules due to the positive and negative charges.

Scientist who pioneered the study of intermolecular forces, leading to van der Waals forces.

Attractions between an ion and a polar molecule, significant in solutions of salts in polar solvents.

Attractions between polar molecules where positive ends attract negative ends.

When an ion distorts the electron cloud of a nonpolar molecule, inducing a dipole.

When a polar molecule induces a dipole in a neighboring nonpolar molecule.

Na⁺ interacts with the negative end of water's dipole, demonstrating ion-dipole forces.

Hydrogen bonds form between NH₃ molecules due to polar nature.