Types of Hydrogen Bonding in Chemistry

False (B)

Lewis symbols or electron dot symbols

<p>covalent</p> Signup and view all the answers

<p>Ionic bond = Electrons are transferred from one atom to another Covalent bond = Electrons are shared equally between atoms Coordinate bond = Electrons are shared, with one atom contributing both electrons</p> Signup and view all the answers

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

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

<p>N with five dots around it</p> Signup and view all the answers

<p>sharing</p> Signup and view all the answers

<p>High melting point = Covalent compound Poor conductor of electricity = Ionic compound Generally gaseous or liquid at room temperature = Covalent compound Usually soluble in water = Ionic compound</p> Signup and view all the answers

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

<p>High melting and boiling points (D)</p> Signup and view all the answers

<p>Good conductors of electricity (B)</p> Signup and view all the answers

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

<p>donor</p> Signup and view all the answers

<p>In HCl, one hydrogen atom shares one electron with one chlorine atom. In H₂O, one oxygen atom shares two electrons with two hydrogen atoms.</p> Signup and view all the answers

<p>Ammonia has a lone pair of electrons on the nitrogen atom, which it donates to the boron atom in BF3, which has an incomplete octet. This sharing of electrons forms a coordinate covalent bond.</p> Signup and view all the answers

<p>Non-polar covalent bond = Sharing of electrons between atoms of different elements Polar covalent bond = Sharing of electrons between atoms of the same element</p> Signup and view all the answers

<p>They have high density (B)</p> Signup and view all the answers

<p>Electronegativity difference and the number of valence electrons.</p> Signup and view all the answers

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

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

<p>Similar electronegativity values of the atoms (D)</p> Signup and view all the answers

<p>hydrogen</p> Signup and view all the answers

<p>Ammonia (NH₃) forms hydrogen bonds due to the presence of a highly electronegative nitrogen atom and a hydrogen atom. These hydrogen bonds are strong intermolecular interactions, leading to a higher boiling point. However, hydrogen chloride (HCl) does not form hydrogen bonds because chlorine is less electronegative than nitrogen. Therefore, HCl's intermolecular forces are weaker, leading to a lower boiling point.</p> Signup and view all the answers

<p>High melting and boiling points = Ionic bond Poor conductors of electricity in the solid state = Covalent bond Soluble in water, insoluble in organic solvents = Ionic bond Directional in nature = Covalent bond</p> Signup and view all the answers

<p>Good conductors of electricity in the solid state (D)</p> Signup and view all the answers

<p>Dipole moment (μ) is a measure of the polarity of a molecule. It is a vector quantity that indicates the magnitude and direction of the separation of positive and negative charges within a molecule. A larger dipole moment indicates a more polar molecule.</p> Signup and view all the answers

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

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

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

<p>Covalent bonds involve the sharing of electrons between atoms, forming a strong bond. Hydrogen bonds are weaker intermolecular forces that arise from the attraction between a partially positive hydrogen atom and a highly electronegative atom.</p> Signup and view all the answers

<p>electronegativity</p> Signup and view all the answers

<p>hydrogen fluoride (HF) (B)</p> Signup and view all the answers

<p>Covalent bond = Formed by sharing electrons between atoms Hydrogen bond = Electrostatic attraction between a partially positive hydrogen atom and a highly electronegative atom Ionic bond = Formed by the transfer of electrons between atoms</p> Signup and view all the answers

<p>Hydrogen bonding is responsible for the unique properties of water, such as its high boiling point, high surface tension, and ability to act as a solvent.</p> Signup and view all the answers

<p>intramolecular</p> Signup and view all the answers

Hydrogen bond between different polar molecules.

Hydrogen bond within the same molecule.

Intermolecular bonds are between different molecules, intramolecular are within one molecule.

Bond formed by sharing electrons between atoms.

Depends on the electronegativity of the bonding atom.

H₂O, HF, NH₃ show intermolecular hydrogen bonding.

Ortho-nitrophenol illustrates intramolecular hydrogen bonding.

Electrostatic attraction between partially positive hydrogen and highly electronegative atom.

A visual representation of an atom's valence electrons using dots around the element symbol.

Electrons in the outermost shell of an atom, involved in forming bonds.

A simplified representation of an element showing its valence electrons as dots around the symbol.

The simplest element with 1 valence electron and symbol H.

Compounds formed by the sharing of electrons between atoms, often displaying characteristic properties.

Usually gases or liquids at room temperature, low melting points, poor conductors, and vary in solubility.

Formed when hydrogen shares its electron with chlorine, completing both their outer shells.

Occurs when two hydrogen atoms bond with one oxygen atom, each sharing electrons for stability.

The association between atoms in a molecule via chemical forces.

A bond formed by the transfer of electrons from one atom to another.

The stable arrangement of electrons similar to noble gases.

Materials that are poor conductors of electricity in solid state.

Attraction between a positively charged hydrogen atom and an electronegative atom.

A strong bond formed by one atom donating both electrons to another atom.

NH₃ has a higher boiling point than HCl due to hydrogen bonding.

A measure of the polarity of a polar covalent bond or molecule.

Covalent compounds are gases or liquids at room temp with low melting points.

Less electronegativity difference; valence electrons are 4-7.

Soft, poor conductors and generally insoluble in polar solvents.

CO₂ forms when carbon shares electrons with oxygen.

The atom that provides the electron pair in a coordinate bond.

The atom that receives the electron pair in a coordinate bond.

A bond formed by equal sharing of electrons between identical atoms.

A bond formed by unequal sharing of electrons between different elements.

Formed from cations and anions; generally crystalline with high densities.