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Questions and Answers
What is ionic bonding?
What is ionic bonding?
The force that holds appropriately charged particles together within a compound.
What are valence electrons?
What are valence electrons?
Electrons in the outermost shell
Which of these elements forms cations?
Which of these elements forms cations?
- Carbon
- Sodium (correct)
- Oxygen
- Chlorine
An endothermic process releases energy.
An endothermic process releases energy.
An exothermic process absorbs energy.
An exothermic process absorbs energy.
What is another name for an ionic compound?
What is another name for an ionic compound?
What does crystal lattice refer to?
What does crystal lattice refer to?
What is lattice energy?
What is lattice energy?
The formation of ionic compounds is an endothermic process.
The formation of ionic compounds is an endothermic process.
Which of the following are characteristics of ionic compounds? (Select all that apply)
Which of the following are characteristics of ionic compounds? (Select all that apply)
How do you write an anion reaction equation?
How do you write an anion reaction equation?
What is electron affinity?
What is electron affinity?
What is ionization energy?
What is ionization energy?
The smaller an atomic radii, the weaker the bond formed.
The smaller an atomic radii, the weaker the bond formed.
The higher the total oxidation charge is for an atom, the weaker the bond formed.
The higher the total oxidation charge is for an atom, the weaker the bond formed.
The stronger the bond, the more positive the lattice energy is for a compound.
The stronger the bond, the more positive the lattice energy is for a compound.
What is oxidation charge?
What is oxidation charge?
Why do brittle ionic solids break apart?
Why do brittle ionic solids break apart?
What is a pseudo noble gas configuration?
What is a pseudo noble gas configuration?
Which of these elements have pseudo noble gas configurations?
Which of these elements have pseudo noble gas configurations?
What configuration do atoms achieve when they bond?
What configuration do atoms achieve when they bond?
How do covalent bonds form?
How do covalent bonds form?
Which of the following are diatomic elements?
Which of the following are diatomic elements?
How many atoms are shared between a single bond? Double? Triple?
How many atoms are shared between a single bond? Double? Triple?
Where is a sigma bond positioned in a bond between two atoms?
Where is a sigma bond positioned in a bond between two atoms?
Why is a sigma bond in the middle of a bond?
Why is a sigma bond in the middle of a bond?
Where is a pi bond located?
Where is a pi bond located?
When can pi bonds occur?
When can pi bonds occur?
What is a Lewis structure?
What is a Lewis structure?
What is resonance?
What is resonance?
What is hybridization?
What is hybridization?
What is the difference between electronegativity and electron affinity?
What is the difference between electronegativity and electron affinity?
Which of the following are exceptions to the octet rule?
Which of the following are exceptions to the octet rule?
Only elements in the second and third periods can have expanded octets.
Only elements in the second and third periods can have expanded octets.
What are Van der Waals forces?
What are Van der Waals forces?
What is dispersion within van der Waals forces?
What is dispersion within van der Waals forces?
What is dipole-dipole within van der Waals forces?
What is dipole-dipole within van der Waals forces?
Where does the dispersion force occur?
Where does the dispersion force occur?
What is hydrogen bonding within van der Waals forces?
What is hydrogen bonding within van der Waals forces?
What are the charged regions of an atom called?
What are the charged regions of an atom called?
What symbols are used to show the charges on each side of a bond?
What symbols are used to show the charges on each side of a bond?
Where does each electronegative symbol (weird s) go?
Where does each electronegative symbol (weird s) go?
The longer the bond length, the stronger the bond.
The longer the bond length, the stronger the bond.
As the number of bonds increase, the bond length decreases.
As the number of bonds increase, the bond length decreases.
What does an electronegative difference of 0 mean?
What does an electronegative difference of 0 mean?
What does an electronegative difference between 0 and 1.70 mean?
What does an electronegative difference between 0 and 1.70 mean?
Which of the following characteristics are true for single bonds?
Which of the following characteristics are true for single bonds?
What are the differences between physical properties of ionic and covalent compounds?
What are the differences between physical properties of ionic and covalent compounds?
What is malleable? Ductile?
What is malleable? Ductile?
Why are there differences between properties of covalent and ionic compounds?
Why are there differences between properties of covalent and ionic compounds?
How many elements have either a weird charge or need roman numerals even though they're not metals?
How many elements have either a weird charge or need roman numerals even though they're not metals?
How many nonmetals need roman numerals?
How many nonmetals need roman numerals?
What five elements need roman numerals even though they're nonmetals?
What five elements need roman numerals even though they're nonmetals?
What three elements have a specific charge even though they're in the metal group? List charge with a dash - Separate with a semicolon
What three elements have a specific charge even though they're in the metal group? List charge with a dash - Separate with a semicolon
What two elements use the prefix system no matter WHAT?
What two elements use the prefix system no matter WHAT?
Flashcards
What is ionic bonding?
What is ionic bonding?
The force that holds appropriately charged particles together within a compound.
What are valence electrons?
What are valence electrons?
electrons in the outermost shell
Which elements form cations?
Which elements form cations?
all metals
What elements form anions?
What elements form anions?
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What is endothermic?
What is endothermic?
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What is exothermic?
What is exothermic?
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What is another name for an ionic compound?
What is another name for an ionic compound?
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What does crystal lattice refer to?
What does crystal lattice refer to?
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What is lattice energy?
What is lattice energy?
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Is the formation of ionic compounds endo or exothermic?
Is the formation of ionic compounds endo or exothermic?
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What are the characteristics of ionic compounds?
What are the characteristics of ionic compounds?
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How do you write an anion reaction equation?
How do you write an anion reaction equation?
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What is electron affinity?
What is electron affinity?
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How do you write a cation reaction equation?
How do you write a cation reaction equation?
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What is ionization energy?
What is ionization energy?
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The smaller an atomic radii,
The smaller an atomic radii,
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The higher the total oxidation charge is for an atom...
The higher the total oxidation charge is for an atom...
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The stronger the bond,
The stronger the bond,
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What is oxidation charge?
What is oxidation charge?
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Why do brittle ionic solids break apart?
Why do brittle ionic solids break apart?
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What is a pseudo noble gas configuration?
What is a pseudo noble gas configuration?
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What elements have pseudo has configurations?
What elements have pseudo has configurations?
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What configuration do atoms achieve when they bond?
What configuration do atoms achieve when they bond?
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How do covalent bonds form?
How do covalent bonds form?
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What are the diatomic elements?
What are the diatomic elements?
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How many atoms are shared between a single bond? Double? Triple?
How many atoms are shared between a single bond? Double? Triple?
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where is a sigma bond positioned in a bind between two atoms?
where is a sigma bond positioned in a bind between two atoms?
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Why is a sigma bond in the middle of a bond?
Why is a sigma bond in the middle of a bond?
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Where is a pi bond located?
Where is a pi bond located?
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When can pi bonds occur?
When can pi bonds occur?
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2,0
2,0
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2,1
2,1
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Study Notes
Ionic Bonding
- Ionic bonding is the attractive force between oppositely charged particles in a compound.
- Metals form cations, nonmetals form anions.
Valence Electrons
- Valence electrons are electrons in the outermost shell of an atom.
Cations and Anions
- Metals form cations (positive ions).
- Nonmetals form anions (negative ions).
Endothermic and Exothermic Reactions
- Endothermic reactions absorb energy.
- Exothermic reactions release energy.
Ionic Compounds (Salts)
- Ionic compounds are also called salts.
- They have a crystal lattice structure.
Lattice Energy
- Lattice energy is the energy needed to separate the ions in an ionic compound.
- Formation of ionic compounds is exothermic because they form stable, low-energy systems.
Properties of Ionic Compounds
- High melting and boiling points.
- Strongest bonds.
- Nonconductors as solids.
- Good conductors when melted or dissolved in water (aqueous solutions).
Formation of Anions
- Anion formation: ELEMENT + e⁻ → ELEMENT⁻¹ + Electron Affinity
Electron Affinity
- Electron affinity is the energy released when an electron attaches to a gaseous atom.
Formation of Cations
- Cation formation: ELEMENT + Ionization Energy → ELEMENT⁺¹ + e⁻
Ionization Energy
- Ionization energy is the energy needed to remove an electron from an atom.
Bond Strength and Atomic Radii
- Smaller atomic radii lead to stronger bonds.
- Higher oxidation charges result in stronger bonds.
- Stronger bonds correspond to more negative lattice energy.
Oxidation Charge
- Oxidation charge is the charge on a monatomic ion.
Ionic Solid Brittleness
- Ionic solids break when ions line up during stress.
Pseudo Noble Gas Configuration
- Pseudo noble gas configurations are relatively stable electron arrangements.
- Elements like copper, silver, and zinc have pseudo noble gas configurations.
Stable Configurations in Bonding
- Atoms achieve a noble gas configuration during bonding.
Covalent Bonding
- Covalent bonds form by sharing electrons.
Diatomic Elements
- Diatomic elements include H₂, N₂, O₂, F₂, Cl₂, Br₂, and I₂.
Bond Types and Number of Shared Electrons
- Single bonds share 2 electrons.
- Double bonds share 4 electrons.
- Triple bonds share 6 electrons.
Sigma and Pi Bonds
- Sigma bonds are located directly between two bonded atoms.
- Pi bonds are located above and below the bond axis.
- Pi bonds only form when there is both a sigma bond and at least one pi bond.
Molecular Geometry and Hybridization
-
Various molecular geometries (linear, bent, trigonal planar, trigonal pyramidal, tetrahedral, trigonal bipyramidal, octahedral) relate to the number of bonding and nonbonding electron pairs. These correlate with specific hybridization (sp, sp², sp³).
-
Key examples are shown in relation to the bonding (e.g., 2,0 is linear, 2,1 is bent).
Dissociation Energy
- Dissociation energy quantifies the energy required to break a bond.
Lewis Structures
- Lewis structures are diagrams representing molecular structures.
Resonance Structures
- Resonance occurs where multiple Lewis structures adequately represent a molecule.
Hybridization
- Hybrid orbitals form from mixing atomic orbitals.
Electronegativity
- Electronegativity measures an atom's ability to attract electrons in a bond.
Electron Affinity
- Electron affinity is the attraction an atom has for an electron.
Exceptions to Octet Rule
- Some molecules (e.g., BH₃, NO₂, ClO₂) do not follow the octet rule, accommodating expanded octets.
Expanded Octets
- Elements in the third period and lower can have expanded octets.
Intermolecular Forces (Van der Waals Forces)
- Intermolecular forces include dispersion, dipole-dipole, and hydrogen bonding.
Dispersion Forces
- Dispersion forces (London Dispersion Forces) are weak intermolecular forces between nonpolar molecules.
- Present in all molecules.
Dipole-Dipole Forces
- Dipole-dipole forces are stronger intermolecular forces between polar molecules.
Hydrogen Bonds
- Hydrogen bonds are strong intermolecular forces between a hydrogen atom of one dipole and a fluorine, oxygen, or nitrogen atom of another dipole.
Polarity and Charges in Bonds
- Polar bonds have partial positive and negative charges (δ+ and δ-).
- Electronegativity differences determine bond polarity.
Bond Length and Strength
- Shorter bonds are generally stronger.
- Increased bond number leads to shorter bond length.
Electronegativity Differences and Bond Types
- Electronegativity differences determine bond types:
- Zero difference: Nonpolar covalent
- 0–1.7: Polar covalent
- 1.7 or greater: Ionic
Bond Length, Strength, and Dissociation Energy (Summary)
- Single bonds: Longest length, weakest strength, least dissociation energy.
- Double bonds: Shorter length, stronger strength, greater dissociation energy.
- Triple bonds: Shortest length, strongest strength, greatest dissociation energy.
Physical Properties of Ionic vs. Covalent Compounds
- Ionic: High melting/boiling points, good aqueous conductors, hard/brittle.
- Covalent: Low melting/boiling points, diverse physical forms, poor conductors.
Malleability and Ductility
- Malleability is the ability to be shaped into sheets.
- Ductility is the ability to be drawn into wires.
Differences in Covalent and Ionic Properties
- Differences stem from the types of attractive forces.
Elements with Variable Charges/Roman Numerals
- Transition metals often have multiple oxidation states.
- Certain nonmetals (e.g., gallium, tin, lead) also require Roman numerals in their compounds' names.
Specific Charges for Some Transition Metals
- Zinc (+2), silver (+1), and cadmium (+2) have consistent charges.
Prefix System Exception Elements
- Antimony and bismuth require the prefix system for representing their specific charges.
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Description
Test your knowledge on ionic bonding, the formation of cations and anions, and the properties of ionic compounds. This quiz covers the basics of ionic interactions, including endothermic and exothermic reactions, and lattice energy concepts.
