Chemistry Chapter 6 Test Answers Flashcards

Podcast Beta

Play an AI-generated podcast conversation about this lesson

Questions and Answers

A ___ is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.

chemical bond

In forming compounds, atoms tend to achieve an octet of electrons in its highest occupied energy level. This is called the ___.

octet rule

A positively charged ion results from ___ electrons.

losing

Negatively charged ions are called ___.

anions Signup and view all the answers

Whether a bond will be ionic or covalent depends on the difference in ___ of the atoms involved.

electronegativity Signup and view all the answers

Ionic compounds are electrically ___.

neutral Signup and view all the answers

___ is the energy released when one mole of an ionic crystalline compound is formed from gaseous ions.

lattice energy Signup and view all the answers

Valence electrons in metal atoms can be modeled as ___.

a sea of electrons Signup and view all the answers

The strength of metallic bonds is given by ___.

enthalpy of vaporization Signup and view all the answers

A ___ bond joins atoms together by sharing electrons.

covalent Signup and view all the answers

A ___ is a neutral group of atoms held together by covalent bonds.

molecule Signup and view all the answers

A ___ is created by equal but opposite charges that are separated by a short distance.

dipole Signup and view all the answers

A charged group of covalently bonded atoms is called a ___.

polyatomic ion Signup and view all the answers

The energy required to break a bond between two covalently bonded atoms is known as the ___.

bond energy Signup and view all the answers

Electrons are shared equally in ____ covalent bonds.

nonpolar Signup and view all the answers

When one atom has a higher electronegativity than the other, a ___ covalent bond will result.

polar Signup and view all the answers

___ forces are forces of attraction between molecules.

intermolecular Signup and view all the answers

Long dispersion forces are the result of the movement of ___.

electrons Signup and view all the answers

Hydrogen bonding can occur when hydrogen is covalently bonded to a highly ___ atom.

electronegative Signup and view all the answers

When two or more valid Lewis structures can be drawn for a molecule, we get what is called ___.

resonance Signup and view all the answers

According to VSEPR theory, what will be the molecular geometry associated with the following types of molecules: AB2E2?

bent Signup and view all the answers

According to VSEPR theory, what will be the molecular geometry associated with the following types of molecules: AB3?

trigonal planar Signup and view all the answers

According to VSEPR theory, what will be the molecular geometry associated with the following types of molecules: AB4?

tetrahedral Signup and view all the answers

According to VSEPR theory, what will be the molecular geometry associated with the following types of molecules: AB3E?

trigonal pyramidal Signup and view all the answers

According to VSEPR theory, what will be the molecular geometry associated with the following types of molecules: AB6?

octahedral Signup and view all the answers

Compare the properties of ionic and molecular compounds.

Ionic compounds have a higher melting point and boiling point. The attraction between the ions is very strong. The melting and boiling point of molecular compounds is low. The bonds between the molecular compounds are weak. Signup and view all the answers

Explain VSEPR theory. What does VSEPR stand for? What roles do shared and unshared pairs of electrons play?

VSEPR is when electrons of different atoms have a greater attraction than those of the same bonded pair. Valence Shell Electron Pair Repulsion. The roles of the shared and unshared electrons play a role in the bonds between the two atoms. Signup and view all the answers

For each of the following types of hybridization, tell me how many orbitals and of what type of hybrid. Also, how many hybrid orbitals are formed: sp?

2 orbitals Signup and view all the answers

For each of the following types of hybridization, tell me how many orbitals and of what type of hybrid. Also, how many hybrid orbitals are formed: sp3?

4 orbitals Signup and view all the answers

For each of the following types of hybridization, tell me how many orbitals and of what type of hybrid. Also, how many hybrid orbitals are formed: sp3d2?

6 orbitals Signup and view all the answers

Describe how the electrons in metallic bonds contribute to the properties of metals.

In contrast to electrons that participate in both ionic and covalent bonds, electrons that participate in metallic bonds delocalize, forming a sea of electrons around the positive nuclei of metals. The availability of 'free' electrons contributes to metals being excellent conductors. Signup and view all the answers

Discuss the role of electronegativity in determining the types of chemical bond formed between atoms.

The greater the difference of electronegativity, the greater the ionic bond is. Below 0.3 = non-polar covalent, 0.3 - 1.7 = polar covalent, 1.7 - 3.3 = ionic. Signup and view all the answers

Study Notes

Chemical Bonds

A chemical bond is a mutual electrical attraction between atom nuclei and valence electrons, which binds atoms together.
Atoms aim to achieve an octet of electrons in their highest occupied energy level, known as the octet rule.

Ions and Charges

A positively charged ion is formed by losing electrons.
Negatively charged ions are referred to as anions.

Bond Types

The type of bond formed (ionic or covalent) depends on the difference in electronegativity between the involved atoms.
Ionic compounds are electrically neutral.
Lattice energy is the energy released when one mole of an ionic crystalline compound forms from gaseous ions.
A covalent bond involves the sharing of electrons between atoms.
A molecule is a neutral group of atoms held together by covalent bonds.

Molecular Properties

A dipole is created by the separation of equal but opposite charges.
A charged group of covalently bonded atoms is identified as a polyatomic ion.
Bond energy is the energy required to break a bond between two covalently bonded atoms.

Covalent Bonding

Nonpolar covalent bonds feature equal sharing of electrons.
Polar covalent bonds occur when one atom has a higher electronegativity than the other.
Intermolecular forces are the attractive forces between molecules.

Electron Movement

Long dispersion forces arise from the movement of electrons.
Hydrogen bonding occurs when hydrogen is covalently bonded to a highly electronegative atom.

Resonance and Structures

Resonance occurs when multiple valid Lewis structures can be drawn for a molecule.

VSEPR Theory

VSEPR theory predicts molecular geometries based on the arrangement of electron pairs around a central atom:
- AB2E2: Bent
- AB3: Trigonal planar
- AB4: Tetrahedral
- AB3E: Trigonal pyramidal
- AB6: Octahedral

Hybridization

sp hybridization involves 2 orbitals.
sp3 hybridization involves 4 orbitals.
sp3d2 hybridization involves 6 orbitals.

Ionic vs. Molecular Compounds

Ionic compounds have higher melting and boiling points due to strong ionic attractions.
Molecular compounds generally have lower melting and boiling points owing to weak intermolecular bonds.

Metallic Bonds

Electrons in metallic bonds are delocalized, forming a sea of electrons surrounding metal nuclei.
The presence of free electrons makes metals excellent conductors of electricity.

Electronegativity

Electronegativity plays a critical role in determining the type of bond formed:
- Below 0.3: Non-polar covalent
- 0.3 - 1.7: Polar covalent
- 1.7 - 3.3: Ionic

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

Reinforce your understanding of chemical bonding and related concepts with these flashcards from Chemistry Chapter 6. Each card presents essential terms and definitions, such as 'chemical bond' and 'octet rule', to help you prepare for your test effectively.