Ionic Bonding and Compounds Quiz

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Questions and Answers

What is ionic bonding?

The force that holds appropriately charged particles together within a compound.

What are valence electrons?

Electrons in the outermost shell.

Which elements form cations?

All metals

What is endothermic?

Energy is absorbed. Signup and view all the answers

What is another name for an ionic compound?

Salt Signup and view all the answers

What does crystal lattice refer to?

The crystalline structure of ionic compounds. Signup and view all the answers

What is lattice energy?

The energy required to separate the ions which compose an ionic compound. Signup and view all the answers

Is the formation of ionic compounds endo or exothermic?

True Signup and view all the answers

What are the characteristics of ionic compounds? (Select all that apply)

Nonconductors as solids Signup and view all the answers

How do you write an anion reaction equation?

ELEMENT + e- -> ELEMENT-1 + electron affinity Signup and view all the answers

What is electron affinity?

The energy released when an electron attaches to an atom in a gaseous state. Signup and view all the answers

What is ionization energy?

The energy required to remove an electron from an atom. Signup and view all the answers

The smaller an atomic radii,

the stronger bond formed Signup and view all the answers

The higher the total oxidation charge is for an atom...

the stronger bond formed. Signup and view all the answers

The stronger the bond,

the more negative lattice energy is for a compound. Signup and view all the answers

What is oxidation charge?

The charge of a monatomic. (One atom ion) Signup and view all the answers

Why do brittle ionic solids break apart?

Their ions line up. Signup and view all the answers

What is a pseudo noble gas configuration?

Relatively stable electron arrangements Signup and view all the answers

What elements have pseudo noble gas configurations?

Elements like Copper, silver, zinc Signup and view all the answers

What configuration do atoms achieve when they bond?

Noble Gas Signup and view all the answers

How do covalent bonds form?

Sharing of electrons Signup and view all the answers

What are the diatomic elements?

H2, N2, O2, F2, Cl2, Br2, I2 Signup and view all the answers

How many atoms are shared between a single bond? Double? Triple?

2, 4, 6 Signup and view all the answers

Where is a sigma bond positioned in a bind between two atoms?

Directly between the two atoms Signup and view all the answers

Why is a sigma bond in the middle of a bond?

The electron orbitals of the two elements overlap, so electrons are completely centred. Signup and view all the answers

Where is a pi bond located?

Above and below a bond Signup and view all the answers

When can pi bonds occur?

When there is either 1 sigma bond and two pi bonds or one sigma bond and one pi bond. Signup and view all the answers

Select the correct combination for 2, 0

Linear, 180, sp Signup and view all the answers

What is a Lewis structure?

A way of showing the structural formula for molecules. Signup and view all the answers

What is resonance?

When a Lewis Structure can be written multiple ways. It occurs when a molecule has one double bond and one or more single bonds of oxygen. Signup and view all the answers

What is hybridization?

When atomic orbitals are mixed to form new, identical hybrid orbitals. Signup and view all the answers

What is the difference between electronegativity and electron affinity?

Electronegativity indicates the ability to attract electrons while electron affinity is the tendency of an atom to accept an electron. Signup and view all the answers

What are the exceptions to the octet rule?

BH3, NO2, ClO2, PCl5, XeF3+ Signup and view all the answers

What elements can have expanded octets?

Elements in the third period or lower. Signup and view all the answers

What are Van der Waals forces?

Intermolecular forces. (Dispersion, dipole-dipole, and hydrogen bonding.) Signup and view all the answers

What is dispersion within van der Waals forces?

The weak intermolecular force between nonpolar molecules. (Sometimes called London Dispersion Force) Signup and view all the answers

What is dipole-dipole within van der Waals forces?

The stronger intermolecular force between polar molecules. Signup and view all the answers

Where does the dispersion force occur?

Between all molecules, but is the only one available for nonpolar molecules. Signup and view all the answers

What is hydrogen bonding within van der Waals forces?

The hydrogen of one dipole (polar bond) and a fluorine, oxygen, or nitrogen of another dipole. Signup and view all the answers

What are the charged regions of an atom called?

Poles and dipoles Signup and view all the answers

What symbols are used to show the charges on each side of a bond?

The delta symbol, δ, which can be δ- (negative) and δ+ (positive) Signup and view all the answers

Where does each electronegative symbol (weird s) go?

The positive one goes on the less electronegative atom and the negative one goes on the more electronegative atom. Signup and view all the answers

The shorter the bond length,

the stronger the bond Signup and view all the answers

As the number of bonds increase,

The bond length decreases. Signup and view all the answers

What does an electronegative difference of 0 mean?

Nonpolar covalent Signup and view all the answers

What does an electronegative difference between 0 and 1.70 mean?

Polar covalent Signup and view all the answers

Which of these options describe the length, strength, and dissociation energy characteristics of single bonds? (Select all that apply)

Least dissociation energy Signup and view all the answers

What are the differences between physical properties of ionic and covalent compounds?

Ionic compounds have high melting and boiling points, are good conductors within aqueous solutions, and are hard/brittle. Covalent compounds have low melting and boiling points, can be molded easily (malleable and ductile), and don't conduct well. Signup and view all the answers

What is malleable? Ductile?

Malleable is when metals can be pressed into flat sheets. Ductile is when metals can be pulled into wires. Signup and view all the answers

Why are there differences between properties of covalent and ionic compounds?

Differences in attractive forces. Signup and view all the answers

How many elements have either a weird charge or need roman numerals even though they're not metals?

10 Signup and view all the answers

How many nonmetals need roman numerals

5 Signup and view all the answers

What five elements need roman numerals even though they're nonmetals

Gallium, Indium, Thallium, Lead, Tin Signup and view all the answers

What three elements have a specific charge even though they're in the metal group? List charge with a dash - Separate with a semicolon

Zinc-+2; Silver-+1; Cadmium-+2 Signup and view all the answers

What two elements use the prefix system no matter WHAT

Antimony and Bismuth Signup and view all the answers

Study Notes

Ionic Bonding

Ionic bonding involves forces attracting oppositely charged particles in a compound.
It's a fundamental interaction holding the compound's structure together.

Valence Electrons

Valence electrons reside in the outermost electron shell.

Cations

Metals form cations.

Anions

Nonmetals form anions.

Endothermic and Exothermic Processes

Endothermic processes absorb energy.
Exothermic processes release energy.

Ionic Compounds (Salts)

Ionic compounds, or salts, are stable low-energy systems.
Their formation is exothermic.

Crystal Lattice Structure

Ionic compounds exhibit a crystalline structure known as a crystal lattice.

Lattice Energy

Lattice energy is the energy needed to separate the ions in a stable ionic compound.

Characteristics of Ionic Compounds

High melting and boiling points
Strong bonds
Nonconducting in solid state
Good conductors in molten or aqueous (water) solutions

Anion Formation

Anion formation involves an element gaining electrons.
Electron affinity is the energy released during that process. (e.g., Element + e⁻ → Element⁻¹ + electron affinity)

Cation Formation

Cation formation involves an element losing electrons.
Ionization energy is the energy required to remove an electron. (e.g., Element + ionization energy → Element⁺¹ + e⁻)

Atomic Radii and Bond Strength

Smaller atomic radii lead to stronger bonds.
Higher total oxidation charge strengthens bonds.
A stronger bond results in a more negative lattice energy.

Oxidation Charge

Oxidation charge represents the charge of a single-atom ion.

Brittleness of Ionic Solids

Ionic solids' brittle nature stems from their regular ion arrangement.

Pseudo Noble Gas Configurations

Some elements exhibit relatively stable electron arrangements, called pseudo noble gas configurations.
Examples include Copper, Silver, and Zinc.

Stable Configurations

Atoms strive for noble gas configurations when bonding.

Covalent Bonding

Covalent bonding arises from the sharing of electrons between atoms.

Diatomic Elements

Diatomic elements, exist as diatomic molecules: H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂.

Bonds and Shared Atoms

Single bonds share 2 atoms, double 4, and triple 6.

Sigma Bonds

Sigma bonds are directly between the bonded atoms.
Electron orbital overlap centers the electrons.

Pi Bonds

Pi bonds lie above and below the sigma bond.

Bond Angles and Hybridization

Specific molecular shapes relate to bond angles and hybridization.

Dissociation Energy

Dissociation energy is the energy needed to break a chemical bond.

Lewis Structures

Lewis structures visually represent molecular structures.

Resonance

Resonance describes multiple equivalent Lewis structures for a molecule.

Hybridization

Hybridization involves mixing atomic orbitals to form equivalent hybrid orbitals.

Electronegativity

Electronegativity measures an atom's ability to attract bonding electrons.

Electron Affinity

Electron affinity is an atom's tendency to gain an electron.

Electronegativity vs. Electron Affinity

Electronegativity reflects attraction within a bond, while electron affinity represents an atom's attraction to a free electron.

Exceptions to the Octet Rule

Certain molecules, like BH₃, and others, don't strictly follow the rule.

Expanded Octets

Elements in the third period and lower occasionally have expanded octets.

Intermolecular Forces (Van der Waals Forces)

Van der Waals forces are intermolecular attractions (dispersion force, dipole-dipole, and hydrogen bonding).

Dispersion Forces

Dispersion forces are the weakest intermolecular force. They occur between all molecules.

Dipole-Dipole Forces

Dipole-dipole forces occur between polar molecules.

Hydrogen Bonding

Hydrogen bonding is a special type of dipole-dipole interaction involving a hydrogen atom bonded to F, O, or N.

Polarity (Poles and Dipoles)

Atoms have charged regions called poles or dipoles.

Electronegativity Differences and Bond Types

Electronegativity differences determine bond types (nonpolar covalent, polar covalent, ionic).

Bond Characteristics

Single bonds are longest, weakest, and have lowest dissociation energy.
Double bonds are shorter, stronger, with higher dissociation energy.
Triple bonds are shortest, strongest, with highest dissociation energy.

Properties of Ionic and Covalent Compounds

Ionic compounds usually have high melting/boiling points, are brittle, and conduct electricity in aqueous solutions.
Covalent compounds generally have low melting/boiling points, are malleable or ductile (can be drawn into wires or hammered), and do not or poorly conduct electricity.

Malleability and Ductility

Malleability refers to the ability to be hammered into thin sheets, while ductility is the ability to be drawn into wires.

Differences in Properties

Differences in properties stem from the difference in attractive forces.

Elements with Unique Charges

Some elements exhibit unusual, specific charges. (e.g., Zinc, Silver, Cadmium)
Specific nonmetals require Roman numerals in their names. (e.g., Lead, Tin)
Some nonmetal elements also need the prefix system, (e.g., Antimony, Bismuth).

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Description

Test your understanding of ionic bonding and the properties of ionic compounds. This quiz covers key concepts such as valence electrons, cations, anions, and the crystalline structure of salts. Explore the differences between endothermic and exothermic processes in relation to ionic compounds.