Chemistry Chapter on Ionic and Metallic Bonds
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Questions and Answers

What is the main reason a large difference in electronegativity causes the formation of an ionic bond?

  • Electrons are transferred from one atom to another. (correct)
  • Atoms repel each other.
  • Electrons are shared between atoms.
  • Atoms form covalent bonds.

Cations are negatively charged ions.

False (B)

What is the chemical formula for calcium chloride?

CaClâ‚‚

Sodium chloride is an example of a compound formed from a reactive metal, sodium, and a gas, __________.

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

Match the following compounds with their correct names:

<p>Na₂CO₃ = Sodium carbonate NH₄C₂H₃O₂ = Ammonium acetate BaCl₂ = Barium chloride Mn(OH)₂ = Manganese(II) hydroxide</p> Signup and view all the answers

Which element has an oxidation number of -2?

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

Noble gases benefit from forming compounds.

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

What is the oxidation number of Carbon (C)?

<p>-4</p> Signup and view all the answers

The compound AlF₃ contains ______ atoms of Aluminum.

<p>1</p> Signup and view all the answers

Match the following characteristics with their respective types of compounds:

<p>Conducts electricity when dissolved in water = Ionic Small electronegativity difference = Covalent Electrons are transferred = Ionic Electrons are shared = Covalent</p> Signup and view all the answers

Which of the following compounds has the formula Au₂(CO₃)₃?

<p>Gold (III) carbonate (A)</p> Signup and view all the answers

In metallic bonds, electrons are transferred from one atom to another.

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

Name an example of an alloy and its component metals.

<p>Bronze, which is made of copper and tin.</p> Signup and view all the answers

The diatomic element Brâ‚‚ is in the state of __________.

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

Match the following properties to their descriptions related to metallic bonds:

<p>Malleability = Ability to be hammered into thin sheets Luster = Shiny appearance Ductility = Ability to be drawn into wires High melting/boiling point = Required energy to change state is high</p> Signup and view all the answers

What is the main characteristic of a polar molecule?

<p>It has partial charges in different locations (A)</p> Signup and view all the answers

Ionic bonds are formed by the sharing of electrons between nonmetals.

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

What is an alloy?

<p>A solution of two or more metals mixed together.</p> Signup and view all the answers

An __________ is formed from losing electrons and has a positive charge.

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

Match the following terms with their definitions:

<p>Electronegativity = Ability of an atom to attract electrons Molecule = Two or more covalently bonded elements Covalent Bond = Sharing of electrons between nonmetals Ion = Atom or group of atoms with an electric charge</p> Signup and view all the answers

Which of the following describes a crystal lattice structure?

<p>Cations and anions are arranged in a repeating pattern (A)</p> Signup and view all the answers

Diatomic elements consist of two different atoms.

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

Define the octet rule.

<p>Atoms will do anything to have 8 valence electrons.</p> Signup and view all the answers

Which of the following represents a polar covalent bond?

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

A double bond involves the sharing of three pairs of electrons.

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

What does VSEPR theory stand for and why is it important in drawing Lewis diagrams?

<p>Valence Shell Electron Pair Repulsion; it helps predict molecular geometry and bond angles.</p> Signup and view all the answers

In a _______ bond, the electrons are shared equally between atoms.

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

Match the following molecules with their corresponding bond type:

<p>H₂ = Nonpolar covalent bond N≡N = Triple bond O=O = Double bond H-H = Single bond</p> Signup and view all the answers

Which chemical formula corresponds to nitrogen trihydride?

<p>NH3 (C)</p> Signup and view all the answers

Diphosphorus trisulfide has the chemical formula P3S2.

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

What is the shape of the molecule H2S?

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

The VSEPR theory helps predict the _____ of a molecule based on electron pair repulsion.

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

Match the acids with their correct names:

<p>HC2H3O2 = Nitrous acid HNO2 = Acetic acid HNO3 = Hydrobromic acid HBr = Nitric acid</p> Signup and view all the answers

Which of the following correctly describes intramolecular forces?

<p>Forces that hold atoms together within a molecule (D)</p> Signup and view all the answers

Covalent bonds are generally associated with high melting and boiling points.

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

What does the statement 'bonding is a spectrum' imply about chemical bonds?

<p>Chemical bonds can vary from ionic to covalent, indicating a range of bond characteristics.</p> Signup and view all the answers

A chemical formula for an ionic compound shows the ratio of ________.

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

Match the following bond types with their corresponding characteristics:

<p>Covalent Bonds = Usually a bad conductor Ionic Bonds = Good conductor in solid state Covalent Compounds = Soft Ionic Compounds = Hard and brittle</p> Signup and view all the answers

Which of the following properties is true for ionic compounds?

<p>They have high boiling points. (C)</p> Signup and view all the answers

Covalent compounds are well-known for being hard and brittle.

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

Explain the main difference between a chemical formula for an ionic compound and a covalent compound.

<p>An ionic compound formula shows the ratio of ions, while a covalent compound formula indicates the composition of the molecule.</p> Signup and view all the answers

Ionic compounds are typically good conductors when in ________ state.

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

Which of the following correctly describes the physical property of covalent compounds?

<p>Poor electrical conductivity (A)</p> Signup and view all the answers

Which of the following molecules is an example of a polar molecule?

<p>Water (Hâ‚‚O) (A)</p> Signup and view all the answers

Nonpolar molecules cannot exhibit any intermolecular forces.

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

What are the three types of intermolecular forces ranked from strongest to weakest?

<p>Hydrogen bonding, Dipole-dipole forces, London Dispersion Forces</p> Signup and view all the answers

The permanent dipoles in polar molecules create _____ intermolecular forces compared to nonpolar molecules.

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

Match the following substances with their dominant intermolecular forces:

<p>H₂O = Hydrogen bonding CO₂ = London Dispersion Forces HI = Dipole-Dipole Fe₂O₃ = Ionic bonding</p> Signup and view all the answers

What factor can lead to nonpolar molecules exhibiting temporary interactions?

<p>Fluctuations in electron distribution (D)</p> Signup and view all the answers

A molecule with a _____ geometry may still be polar if the bond polarities do not cancel out due to symmetry.

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

London Dispersion Forces are the strongest type of intermolecular force.

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

Flashcards

Chemical Bond

A force that holds atoms together in a substance.

Electronegativity

The ability of an atom to attract electrons in a bond.

Octet Rule

The tendency of atoms to have 8 valence electrons, like a full set.

Covalent Compound

A compound formed when two or more elements share electrons.

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Ionic Compound

A compound formed when electrons are transferred from a metal to a nonmetal.

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Intermolecular Forces

The attractive forces between particles in a substance.

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Viscosity

A fluid's resistance to movement.

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Boiling Point

The amount of energy needed to overcome attractions between particles in a liquid.

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Electronegativity and Ionic Bonds

The ability of an atom to attract electrons in a chemical bond. A larger difference in electronegativity between two atoms leads to a transfer of electrons, forming an ionic bond.

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What are Cations?

Positively charged ions formed when an atom loses electrons.

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What are Anions?

Negatively charged ions formed when an atom gains electrons.

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Binary Ionic Compounds

A compound formed from one metal and one nonmetal.

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Compounds with Polyatomic Ions

A compound formed from one metal and a polyatomic ion.

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Why don't noble gases form compounds?

Noble gases do not benefit from forming compounds because they have a full outer shell of electrons, making them very stable.

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What is the difference between ionic and covalent bonds?

Ionic compounds are formed when a metal transfers electrons to a nonmetal, resulting in a positive and negative ion that attract each other. Covalent compounds involve nonmetals sharing electrons.

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What is oxidation number?

The oxidation number of an element indicates its charge when it forms an ion. It can be positive, negative, or zero.

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How do you determine the elements and number of atoms in a compound?

The elements and their respective numbers of atoms in a compound determine its chemical formula.

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How does electronegativity affect bonding?

The electronegativity difference between two atoms determines whether they will form an ionic or covalent bond. A large difference indicates an ionic bond, while a small difference indicates a covalent bond.

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Bonding Spectrum

The character of bonds can vary, from purely ionic to purely covalent, with many bonds falling somewhere in between.

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Chemical Reaction

The process of forming or breaking chemical bonds between atoms, resulting in changes to the chemical makeup of substances.

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Molecule

A group of two or more atoms held together by chemical bonds.

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Compound

A substance formed from two or more different elements chemically combined in a fixed ratio.

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Covalent Bonds

Chemical bonds formed by the sharing of electrons between atoms.

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Ionic Bonds

Chemical bonds formed by the transfer of electrons from one atom to another, resulting in oppositely charged ions that attract each other.

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Ionic Formula

A chemical formula that represents the ratio of ions present in a compound, but does not indicate the actual number of atoms.

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Covalent Formula

A chemical formula that represents the actual number and types of atoms present in a molecule.

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Nonpolar covalent bond

A type of covalent bond where electrons are shared equally between two atoms, leading to a neutral charge distribution.

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Polar covalent bond

A type of covalent bond where electrons are shared unequally between two atoms, resulting in a partial positive and partial negative charge.

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VSEPR theory

The theory that predicts the shape of molecules based on the repulsion between electron pairs around a central atom.

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Lewis structure

A diagram that represents the arrangement of atoms and valence electrons in a molecule.

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What distinguishes metallic bonds from ionic and covalent bonds?

Metallic bonds differ from ionic and covalent bonds because electrons in metallic bonds are delocalized, meaning they can move freely throughout the metal structure. In ionic bonds, electrons are transferred from one atom to another, while in covalent bonds, electrons are shared between atoms.

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Why do metallic bonds form a 'sea of electrons'?

The 'sea of electrons' in metallic bonds is formed because the valence electrons of metal atoms are loosely held. This allows electrons to move freely, making metals good conductors of electricity.

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What properties are unique to metals due to their bonding?

Metals are malleable (can be hammered into sheets), ductile (can be drawn into wires), lustrous (shiny), and have high melting and boiling points. These properties are all due to the strong metallic bonds and the delocalized electrons.

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What is an alloy? Give an example and explain its use.

An alloy is a mixture of two or more metals. For example, bronze is an alloy composed of copper and tin. Its strength and durability make it suitable for various applications, such as building.

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How does electronegativity affect the formation of covalent bonds?

Electronegativity, the tendency of an atom to attract electrons, plays a key role in determining how atoms share electrons in covalent bonds. Atoms with similar electronegativity will share electrons equally, while atoms with different electronegativity will share electrons unequally, leading to polar covalent bonds.

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Electron Domain

A region of electron density around a central atom, including single, double, or triple bonds, and lone pairs of electrons.

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Molecular Shape

The molecular shape where electron domains are arranged around a central atom to minimize electron-electron repulsion.

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Polar molecule

A molecule with a positive and negative end due to uneven electron distribution.

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Nonpolar molecule

A molecule with an even electron distribution, causing no distinct positive or negative ends.

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Electronegativity and bond polarity

The difference in electronegativity between bonded atoms determines the direction of electron sharing, leading to a polar or nonpolar bond.

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Symmetry and molecular polarity

Even if individual bonds are polar, a molecule can be nonpolar if its symmetrical shape cancels out the polarities.

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Intermolecular forces and boiling point

Stronger intermolecular forces result in higher boiling points because more energy is needed to overcome the attractions between molecules.

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London Dispersion Forces (LDF)

The weakest intermolecular force, arising from temporary dipoles due to fluctuating electron distribution.

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Intermolecular forces and viscosity

Stronger intermolecular forces lead to higher viscosities because the molecules are more strongly attracted and resist flowing.

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Hydrogen bonding

The strongest intermolecular force, involving a hydrogen atom bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine).

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