Chemistry Flashcards - Bonding Types

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Questions and Answers

What is ionic bonding?

A covalent bond with equally attracted electrons.

A force that attracts electrons from one atom to another. (correct)

A bond formed when atoms share electrons.

A bond where charges are separated.

What is covalent bonding?

A bond that forms between oppositely charged ions.

A force that attracts electrons.

A bond where positive and negative charges are separated.

A bond formed when atoms share electrons. (correct)

What is a non-polar covalent bond?

A covalent bond in which the bonding electrons are equally attracted to both bonded atoms.

What does it mean when a molecule is described as polar?

It means the positive and negative charges are separated within the molecule. Signup and view all the answers

What is a polar covalent bond?

A covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom. Signup and view all the answers

Define a molecule.

The smallest unit of a substance that keeps all of the physical and chemical properties of that substance. Signup and view all the answers

What is a molecular formula?

A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms. Signup and view all the answers

What is bond energy?

The energy required to break the bonds in 1 mol of a chemical compound. Signup and view all the answers

What is electron dot notation?

An electron-configuration notation where only the valence electrons of an atom are shown. Signup and view all the answers

What is a Lewis structure?

A structural formula in which electrons are represented by dots. Signup and view all the answers

What is a single bond?

A covalent bond in which two atoms share one pair of electrons. Signup and view all the answers

What are multiple bonds?

Bonds in which the atoms share more than one pair of electrons. Signup and view all the answers

What is resonance?

The bonding in molecules or ions that cannot be correctly represented by a single Lewis structure. Signup and view all the answers

What is an ionic compound?

A compound composed of ions bound together by electrostatic attraction. Signup and view all the answers

What is lattice energy?

The energy associated with constructing a crystal lattice relative to the energy of constituent atoms. Signup and view all the answers

What is a polyatomic ion?

An ion made of two or more atoms. Signup and view all the answers

What is metallic bonding?

A bond formed by the attraction between positively charged metal ions and the electrons around them. Signup and view all the answers

What is VSEPR theory?

A theory that predicts some molecular shapes based on electron pairs repelling each other. Signup and view all the answers

What distinguishes ionic from covalent bonding?

Ionic bonding results from electrical attraction between cations and anions, while covalent bonding arises from shared electron pairs. Signup and view all the answers

How is electronegativity used in bond character determination?

It is based on the difference in electronegativities; 0-0.3 is non-polar covalent, 0.31-1.7 is polar covalent, and 1.7-3.3 is ionic. Signup and view all the answers

What types of bonding occur between atoms?

Ionic, covalent, and metallic bonding. Signup and view all the answers

What is hybridization?

A model explaining how atomic orbitals merge to form new hybrid orbitals during bond formation. Signup and view all the answers

What is the octet rule?

The rule that states atoms tend to form bonds so that each atom has eight electrons in its highest occupied energy level. Signup and view all the answers

Why are ionic compounds generally harder and more brittle?

Due to the strong electrostatic forces between ions in the crystal lattice. Signup and view all the answers

What accounts for the high electrical conductivity of metals?

The freedom of electrons to move in a network of metal atoms. Signup and view all the answers

Study Notes

Bonding Concepts

Ionic Bonding: Involves attraction between cations and anions, resulting in the formation of ions from neutral atoms.
Covalent Bonding: Characterized by the sharing of one or more pairs of electrons between atoms.
Polar and Nonpolar Covalent Bonds:
- Nonpolar occurs when electrons are equally shared, while polar has an unequal distribution, leading to positive and negative charges within the molecule.

Molecular Structure

Molecule: Smallest unit retaining physical and chemical properties of a substance; can consist of one or multiple atoms.
Molecular Formula: Indicates the types and numbers of atoms in a molecule without showing their arrangement.
Lewis Structure: Represents atoms and bonding; electrons shown as dots. Pairs in bonds represented by dashed lines or paired dots.

Bond Energy

Bond Energy: Energy required to break bonds in one mole of a substance, indicating bond strength.
Single, Double, and Triple Bonds: Single bonds share one electron pair, double bonds two, and triple bonds three, with triple bonds being the strongest.

Resonance and Ionic Compounds

Resonance: Describes molecules or ions that can't be depicted by a single Lewis structure.
Ionic Compounds: Formed by the electrostatic attraction between positive and negative ions; generally have higher melting and boiling points compared to molecular compounds.

Lattice Energy

Lattice Energy: Energy related to the formation of a crystal lattice from gaseous ions; stronger bonding indicates greater lattice energy and stability.

Electron Configuration Notation

Electron Dot Notation: Visual representation of valence electrons around an element’s symbol to determine bonding potential.

VSEPR Theory

VSEPR Theory: Predicts molecular shapes based on electron pair repulsion around a central atom.
- Common geometries: linear (AB2), trigonal planar (AB3), tetrahedral (AB4), trigonal pyramidal (AB5), and octahedral (AB6).

Hybridization

Hybridization: Concept where atomic orbitals mix to form new hybrid orbitals for bond formation, with examples including sp3 for tetrahedral arrangements.

Conductivity and Physical Properties

Metals as Conductors: Their high electrical conductivity is due to the presence of a "sea of electrons" which can freely move and conduct electricity.
Metal Properties: Metals are malleable and ductile; they can deform under stress without breaking due to non-directional metallic bonding.

Comparisons and Characteristics

Comparative Bonding: Ionic bonds are typically stronger and result in compounds with higher melting points compared to molecular bonds, which tend to exhibit lower boiling and melting points.
Conductivity Comparison: Ionic compounds do not conduct electricity in solid form but do when dissolved or melted.

Stability and Chemical Bonding

Bonding Stability: Atoms chemically bond to achieve lower potential energy and greater stability, influenced by the octet rule which dictates that atoms tend to complete their outer shells with eight electrons.
Factors Affecting Geometry: Includes the presence of double/triple bonds and the arrangement of lone pairs around the central atom.

Molecular vs Ionic Compounds

Basic Units: Molecular compounds consist of molecules while ionic compounds are composed of ions that maintain electrical neutrality.

Relating Lattice Energy to Compound Properties

Stronger ionic bonding results in higher lattice energy, with implications for melting and boiling points among various ionic compounds.

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Description

This quiz on chemistry flashcards focuses on the different types of bonding, including ionic, covalent, and polar covalent bonds. Each flashcard provides a definition to help you understand these essential concepts in chemistry.