Chemistry Chapter 8 Test Flashcards

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Questions and Answers

What is a covalent bond?

  • A chemical bond that results from the sharing of valence electrons (correct)
  • A bond between a metal and a nonmetal
  • A bond that does not involve electrons
  • A bond formed by the transfer of electrons

What forms when two or more atoms covalently bond?

Molecule

What is a formula unit?

The simplest ratio of ions represented in an ionic compound.

What does a Lewis structure represent?

<p>A model that uses electron-dot structures to show how electrons are arranged in molecules.</p> Signup and view all the answers

What is a sigma bond?

<p>A single covalent bond formed when an electron pair is shared by the direct overlap of bonding orbitals.</p> Signup and view all the answers

What is a pi bond?

<p>A bond formed when parallel orbitals overlap to share electrons.</p> Signup and view all the answers

What is an exothermic reaction?

<p>A chemical reaction in which more energy is released than is required to break bonds in the initial reactants.</p> Signup and view all the answers

What is an endothermic reaction?

<p>A chemical reaction in which a greater amount of energy is required to break the existing bonds than is released when new bonds form.</p> Signup and view all the answers

What is an oxyacid?

<p>Any acid that contains hydrogen and an oxyanion.</p> Signup and view all the answers

What is a structural formula?

<p>A molecular model that shows relative positions of atoms using symbols and bonds.</p> Signup and view all the answers

What is resonance?

<p>A condition that occurs when more than one valid Lewis structure exists for the same molecule.</p> Signup and view all the answers

What is a coordinate covalent bond?

<p>Forms when one atom donates a pair of electrons to share with another atom.</p> Signup and view all the answers

What is the VSEPR model?

<p>Valence Shell Electron Pair Repulsion model.</p> Signup and view all the answers

What is hybridization?

<p>A process in which atomic orbitals are mixed to form new, identical hybrid orbitals.</p> Signup and view all the answers

What is a polar covalent bond?

<p>A type of bond that forms when electrons are not shared equally.</p> Signup and view all the answers

What are diatomic molecules?

<p>Molecules composed only of two atoms.</p> Signup and view all the answers

What are multiple bonds?

<p>Form when atoms need to share more than one pair of electrons to achieve noble gas configuration.</p> Signup and view all the answers

What are single bonds?

<p>When two atoms share one pair of electrons.</p> Signup and view all the answers

What determines bond strength?

<p>Bond strength is determined by bond length.</p> Signup and view all the answers

Forming bonds _______ energy, breaking bonds _______ energy.

<p>requires, releases</p> Signup and view all the answers

What is bond dissociation energy?

<p>The amount of energy necessary to break a bond.</p> Signup and view all the answers

What elements are diatomic when alone?

<p>Br I N Cl H O F</p> Signup and view all the answers

What is nomenclature in chemistry?

<p>The rules applied for naming compounds.</p> Signup and view all the answers

What is the bond angle for a linear shaped molecule?

<p>180 degrees</p> Signup and view all the answers

What is the bond angle for a bent or angular shaped molecule?

<p>104.5 degrees</p> Signup and view all the answers

What is the bond angle for a trigonal planar shaped molecule?

<p>120 degrees</p> Signup and view all the answers

What is the bond angle for a trigonal pyramid shaped molecule?

<p>107.3 degrees</p> Signup and view all the answers

What is the bond angle for a tetrahedral shaped molecule?

<p>109.5 degrees</p> Signup and view all the answers

When a bond is non-polar covalent, its electronegativity is _____.

<p>0 - 0.4</p> Signup and view all the answers

When a bond is polar covalent, its electronegativity is _____.

<p>0.5 - 1.6</p> Signup and view all the answers

When a bond is ionic, its electronegativity is _____.

<p>Greater than or equal to 1.7</p> Signup and view all the answers

What is an exception to the octet rule?

<p>Odd number of valence electrons</p> Signup and view all the answers

What is a sub-octet?

<p>Less than eight electrons but the central atom is still satisfied.</p> Signup and view all the answers

What is an expanded octet?

<p>More than eight electrons but the central atom is still satisfied.</p> Signup and view all the answers

How many sigma and/or pi bonds does a single bond have?

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

How many sigma and/or pi bonds does a double bond have?

<p>1 Sigma, 1 Pi</p> Signup and view all the answers

How many sigma and/or pi bonds does a triple bond have?

<p>1 Sigma, 2 Pi</p> Signup and view all the answers

What does the prefix 'Mono-' signify?

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

What does the prefix 'Di-' signify?

<p>2</p> Signup and view all the answers

What does the prefix 'Tri-' signify?

<p>3</p> Signup and view all the answers

What does the prefix 'Tetra-' signify?

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

What does the prefix 'Penta-' signify?

<p>5</p> Signup and view all the answers

What does the prefix 'Hexa-' signify?

<p>6</p> Signup and view all the answers

What does the prefix 'Hepta-' signify?

<p>7</p> Signup and view all the answers

What does the prefix 'Octa-' signify?

<p>8</p> Signup and view all the answers

What does the prefix 'Nona-' signify?

<p>9</p> Signup and view all the answers

What does the prefix 'Deca-' signify?

<p>10</p> Signup and view all the answers

What is a binary acid?

<p>The first word has the prefix hydro- and the rest of the first word consists of a form of the root of the second element plus the suffix -ic.</p> Signup and view all the answers

What ending do you use for a binary acid?

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

What is the suffix change for an oxyacid that ends with -ate?

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

What ending do you use for a binary acid that ends with -ite?

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

What is electronegativity?

<p>The relative tendency of an atom to attract shared pairs of electrons.</p> Signup and view all the answers

With hybridization, when a s^2 becomes _____.

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

With hybridization, when a s^2p^1 becomes _____.

<p>sp^2</p> Signup and view all the answers

With hybridization, when a s^2p^2 becomes _____.

<p>sp^3</p> Signup and view all the answers

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Study Notes

Covalent Bonds and Molecules

  • Covalent Bond: Formed by sharing valence electrons; typically between nonmetals.
  • Molecule: Group of two or more atoms bonded covalently; lower potential energy than individual atoms.
  • Multiple Bonds: Atoms share more than one pair of electrons for noble gas configuration.
  • Single Bonds: involve sharing one pair of electrons (sigma bond).
  • Bond Strength: Related to bond length; shorter bonds are generally stronger (e.g., double and triple bonds).

Ionic Compounds and Their Representation

  • Formula Unit: Represents the simplest ratio of ions in an ionic compound.
  • Nomenclature: Uses prefixes for compounds formed from nonmetals, diverging from ionic compound rules.

Structural Representations

  • Lewis Structure: Visual representation of electron arrangements in molecules using dots and lines.
  • Structural Formula: Depicts relative atom positions using symbols and bonds; derived from Lewis structures.

Types of Bonds

  • Sigma Bond: First bond formed between atoms through direct orbital overlap.
  • Pi Bond: Formed by parallel orbital overlap when electrons are shared.
  • Coordinate Covalent Bond: Created when one atom donates a pair of electrons for bonding.

Energetics of Reactions

  • Exothermic Reaction: More energy released than needed for bond-breaking; heat released.
  • Endothermic Reaction: More energy required to break bonds than what is released during bond formation; heat absorbed.

Electron Pair Arrangement and Bond Angles

  • VSEPR Model: Predicts molecular shape based on minimizing electron pair repulsion.
  • Bond Angles:
    • Linear: 180 degrees
    • Bent: 104.5 degrees
    • Trigonal Planar: 120 degrees
    • Trigonal Pyramid: 107.3 degrees
    • Tetrahedral: 109.5 degrees

Electronegativity and Bond Polarity

  • Electronegativity Scale:
    • Non-polar Covalent (0 - 0.4)
    • Polar Covalent (0.5 - 1.6)
    • Ionic (≥1.7)
  • Polar Covalent Bond: Electrons are not shared equally between atoms.

Exceptions to the Octet Rule

  • Odd Number of Valence Electrons: Causes difficulty in achieving a stable state.
  • Sub-Octet: Central atom has fewer than eight electrons but is satisfied.
  • Expanded Octet: Central atom has more than eight electrons but maintains stability.

Hybridization

  • Hybridization Processes: Mixing of atomic orbitals to form hybrid orbitals.
  • Types:
    • sp: From s²
    • sp²: From s²p¹
    • sp³: From s²p²

Additional Key Terms and Concepts

  • Bond Dissociation Energy: Energy needed to break a bond; higher for stronger bonds.
  • Diatomic Molecules: Consist of two atoms; can be the same or different elements (Br, I, N, Cl, H, O, F).
  • Binary Acids: Named with the prefix hydro- and using -ic suffix for -ate and -ous for -ite in oxyacids.

Common Prefixes for Molecular Compounds

  • Mono-: 1
  • Di-: 2
  • Tri-: 3
  • Tetra-: 4
  • Penta-: 5
  • Hexa-: 6
  • Hepta-: 7
  • Octa-: 8
  • Nona-: 9
  • Deca-: 10

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