Chemistry: Covalent and Ionic Bonds Quiz

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

<p>0 (C)</p> Signup and view all the answers

<p>Step 3 (B)</p> Signup and view all the answers

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

<p>Only double bonds (B)</p> Signup and view all the answers

<p>0 (A)</p> Signup and view all the answers

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

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

<p>Both electrons come from the same atom (D)</p> Signup and view all the answers

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

<p>Valence electrons - Lone pairs - 1/2(Bonding pairs) (D)</p> Signup and view all the answers

<p>One double bond and two single bonds (C)</p> Signup and view all the answers

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

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

<p>$PCl_5$ (D)</p> Signup and view all the answers

<p>Side-to-side overlapping (D)</p> Signup and view all the answers

<p>3s, 3p, and 3d (C)</p> Signup and view all the answers

<p>Overlapping of atomic orbitals (A)</p> Signup and view all the answers

<p>$sp^3$ (C)</p> Signup and view all the answers

<p>$1s^2 2s^2 2p^1$ (B)</p> Signup and view all the answers

<p>They can expand their octet. (A)</p> Signup and view all the answers

<p>Polar covalent bond (B)</p> Signup and view all the answers

<p>The dipoles cancel each other out. (A)</p> Signup and view all the answers

<p>To accurately describe a molecule when one structure is insufficient. (B)</p> Signup and view all the answers

<p>$N ext{-} N$ has a bond order of 3, $O ext{-} O$ has a bond order of 2. (C)</p> Signup and view all the answers

<p>$SO_2$ (D)</p> Signup and view all the answers

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

<p>Covalent bonds involve the sharing of electrons. (D)</p> Signup and view all the answers

<p>The dipole moments in $NF_3$ cancel each other due to their directional movements. (C)</p> Signup and view all the answers

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

<p>The repulsion between electron pairs in the valence shell (B)</p> Signup and view all the answers

<p>The molecule contains axial and equatorial bonds. (A), It exhibits a trigonal bipyramidal geometry. (C)</p> Signup and view all the answers

<p>109.5° (B)</p> Signup and view all the answers

<p>$H_2O$ has a V-shaped or bent geometry. (C)</p> Signup and view all the answers

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

<p>120° (A)</p> Signup and view all the answers

A chemical bond formed by the sharing of valence electrons between two atoms.

A chemical bond formed by the transfer of valence electrons from one element to another, usually between a metal and a non-metal.

A visual representation of the distribution of electrons in a molecule.

The number of valence electrons an atom 'owns' in a molecule.

A type of covalent bond where two atoms share a single pair of electrons.

A type of covalent bond where two atoms share two pairs of electrons.

A type of covalent bond where two atoms share three pairs of electrons.

The representation of the electron distribution in a molecule based on its Lewis structure.

The octet rule states that atoms tend to gain, lose or share electrons to achieve a stable configuration with eight electrons in their valence shell, similar to noble gases.

Molecules or ions that do not follow the octet rule, having an odd number of valence electrons or less than eight electrons in their valence shell, are called exceptions to the octet rule.

Bond parameters are a set of characteristics that describe the properties of a chemical bond, including bond length, bond energy, bond angle, and bond order.

Bond length is the average distance between the nuclei of two bonded atoms. It depends on the size and type of atoms involved.

Bond energy is the amount of energy required to break a bond between two atoms. It's a measure of bond strength.

Bond angle is the angle between two adjacent bonds, usually measured in degrees. It describes the shape of a molecule.

Bond order is the number of electron pairs shared between two atoms. It indicates the strength of the bond.

Resonance is a phenomenon where a single Lewis structure cannot accurately represent a molecule due to electron delocalization. Multiple structures are drawn with similar energies, and a hybrid structure is used to describe the molecule accurately.

A positively charged ion formed by the addition of a proton (H+) to a water molecule (H2O).

A positively charged ion formed when ammonia (NH3) accepts a proton (H+).

A negatively charged ion composed of one carbon atom and three oxygen atoms. It has a charge of -2.

A negatively charged ion made up of one nitrogen atom and three oxygen atoms. It has a charge of -1

A negatively charged ion made of one nitrogen and two oxygen atoms. It has a charge of -1.

A molecule consisting of three oxygen atoms. The central oxygen atom has a formal charge of 0, while the terminal oxygen atoms have a formal charge of -1.

A type of covalent bond where both electrons in the bond come from the same atom. This occurs when one atom has a lone pair of electrons and the other atom needs to gain an electron.

The theory explaining the shape of molecules based on minimizing repulsion between electron pairs in the valence shell.

The number of electron pairs around a central atom, including both bonding pairs and lone pairs.

A molecule with two bonding pairs and no lone pairs, resulting in a 180° bond angle.

A molecule with three bonding pairs and no lone pairs, resulting in 120° bond angles between the bonded atoms.

A molecule with four bonding pairs and no lone pairs, resulting in 109.5° bond angles between the bonded atoms.

A molecule with four bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.

A molecule with five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal shape.

A molecule with six bonding pairs and no lone pairs, resulting in an octahedral shape.

A type of covalent bond formed by the overlapping of atomic orbitals along the internuclear axis, resulting in a strong bond.

A type of covalent bond formed by the overlapping of atomic orbitals side-by-side, resulting in a weaker bond.

The process of mixing different atomic orbitals of an atom to form new hybrid orbitals with different shapes and energies.

A type of hybridization involving one s and one p orbital, resulting in two sp hybrid orbitals.

A type of hybridization involving one s and two p orbitals, resulting in three sp² hybrid orbitals.

A type of hybridization involving one s and three p orbitals, resulting in four sp³ hybrid orbitals.

A type of hybridization involving one s, three p, and one d orbital, resulting in five sp³d hybrid orbitals.

A type of hybridization involving one s, three p, and two d orbitals, resulting in six sp³d² hybrid orbitals.