Chemistry Bonding Unit Quiz
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Questions and Answers

What does the suffix 'ic' indicate about a metal's oxidation state?

  • It indicates a neutral state.
  • It indicates a higher oxidation state. (correct)
  • It indicates no oxidation state.
  • It indicates a lower oxidation state.

Which of the following correctly pairs a metal with its old name based on oxidation state?

  • Ferric = Fe+2
  • Cuprous = Cu+2
  • Cupric = Cu+2 (correct)
  • Ferrous = Fe+3

What type of bond is formed between nonmetals?

  • Dual bond
  • Covalent bond (correct)
  • Ionic bond
  • Metallic bond

Which of the following best describes a nonpolar covalent bond?

<p>Electrons are shared equally. (D)</p> Signup and view all the answers

What is the primary factor that determines whether electrons are shared equally or unequally in a covalent bond?

<p>Electronegativity of the atoms (B)</p> Signup and view all the answers

Which element has the highest electronegativity?

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

What does the term 'BARF' stand for in the context of bonding?

<p>Break, Absorb, Release, Form (A)</p> Signup and view all the answers

How many electrons are involved in forming one covalent bond?

<p>2 electrons (D)</p> Signup and view all the answers

What type of bond is formed between two nonmetals sharing electrons equally?

<p>Nonpolar covalent bond (A)</p> Signup and view all the answers

Which of the following bonds has the strongest bond energy?

<p>Triple bond (D)</p> Signup and view all the answers

What type of bond exists between the elements in the molecule HCl?

<p>Polar covalent bond (B)</p> Signup and view all the answers

In MgSO4, what types of bonding are present?

<p>Both ionic and covalent bonding (A)</p> Signup and view all the answers

What distinguishes polar covalent bonds from nonpolar covalent bonds?

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

What is a coordinate covalent bond?

<p>A bond where both electrons come from the same atom (C)</p> Signup and view all the answers

Which of the following molecules is an example of a diatomic molecule with a nonpolar bond?

<p>Cl2 (D)</p> Signup and view all the answers

Which statement is true regarding bond length and bond strength?

<p>Stronger bonds have shorter lengths (D)</p> Signup and view all the answers

What type of bond exists when two atoms have the same electronegativity value?

<p>Nonpolar covalent bond (A)</p> Signup and view all the answers

Which of the following pairs of atoms will form a polar covalent bond?

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

What does the electronegativity difference indicate about the bond between two atoms?

<p>It influences the electron sharing between the atoms. (B)</p> Signup and view all the answers

Which of the following molecules is most likely to be a nonpolar covalent molecule?

<p>O2 (A)</p> Signup and view all the answers

Which diatomic molecule shares four electrons between its two atoms?

<p>O2 (D)</p> Signup and view all the answers

What characteristic is NOT true about nonpolar covalent bonds?

<p>They form between atoms of different electronegativities. (B)</p> Signup and view all the answers

In a covalent bond, each bond typically consists of which number of electrons?

<p>2 (A)</p> Signup and view all the answers

What type of bond shares electrons unequally?

<p>Polar covalent bond (C)</p> Signup and view all the answers

What happens when a bond is formed between atoms?

<p>Energy is released. (C)</p> Signup and view all the answers

Which type of bond involves the transfer of electrons?

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

What is the primary reason atoms form compounds?

<p>To achieve a stable octet of valence electrons (C)</p> Signup and view all the answers

Which of the following accurately describes metals in terms of bonding?

<p>Metals possess a 'sea of freely moving electrons'. (C)</p> Signup and view all the answers

Which statement is true about the octet rule?

<p>Hydrogen and helium cannot satisfy the octet rule. (D)</p> Signup and view all the answers

What is the relationship between bond formation and potential energy?

<p>Bond formation decreases potential energy. (D)</p> Signup and view all the answers

What defines a binary compound?

<p>A compound formed from two different elements. (D)</p> Signup and view all the answers

What is the main characteristic of anions?

<p>They are negatively charged ions. (C)</p> Signup and view all the answers

Which statement correctly explains why MgBr2 is classified as an ionic compound?

<p>Mg is a metal and Br is a nonmetal. (A)</p> Signup and view all the answers

What constitutes a salt in the context of ionic compounds?

<p>An ionic compound where H+ is not the positive ion. (A)</p> Signup and view all the answers

How do metals typically form positive ions?

<p>By losing their valence electrons. (A)</p> Signup and view all the answers

What does a Roman numeral signify in the name of a metal ion?

<p>The oxidation state of the metal ion. (A)</p> Signup and view all the answers

What is true about monatomic nonmetal ions?

<p>They gain electrons to form negative ions. (A)</p> Signup and view all the answers

Which of the following is a characteristic of polyatomic ions?

<p>They are charged groups of covalently bonded atoms. (A)</p> Signup and view all the answers

What happens when there is no number next to the charge of a polyatomic ion?

<p>The charge is assumed to be 1. (C)</p> Signup and view all the answers

How is ammonium classified in relation to other ions?

<p>It is considered an honorary metal. (A)</p> Signup and view all the answers

Which statement correctly describes the relationship between intermolecular forces (IMFs) and boiling points?

<p>Stronger IMFs result in higher boiling points. (C)</p> Signup and view all the answers

What is a characteristic of metallic bonding?

<p>Metal atoms are surrounded by a sea of freely moving electrons. (D)</p> Signup and view all the answers

Under what condition do ionic compounds conduct electricity?

<p>When melted or dissolved in water. (C)</p> Signup and view all the answers

Which type of bonding is likely to result in the highest melting points?

<p>Ionic bonding. (B)</p> Signup and view all the answers

Which end of a water (H2O) molecule is slightly positive?

<p>The hydrogen end. (B)</p> Signup and view all the answers

Why do covalent substances typically not conduct electricity?

<p>They lack freely moving charged particles. (A)</p> Signup and view all the answers

What happens to the boiling point of a substance if the intermolecular forces are weakened?

<p>It decreases. (B)</p> Signup and view all the answers

Which of the following substances has the strongest intermolecular forces?

<p>A solid ionic compound. (A)</p> Signup and view all the answers

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Flashcards

Covalent bond

A chemical bond formed by the sharing of electron pairs between atoms.

Ionic bond

A chemical bond formed by the electrostatic attraction between oppositely charged ions.

Metallic bond

A chemical bond formed by the attraction between metal ions and free electrons.

Octet rule

Atoms gain, lose, or share electrons to achieve eight electrons in their outer shell.

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Bond formation

Energy is released when a bond is formed.

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Bond breaking

Energy is absorbed when a bond is broken.

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Electronegativity

A measure of an atom's ability to attract electrons in a chemical bond.

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Compound

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

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What does the suffix "ic" indicate in a chemical name?

The higher oxidation state of a metal in a compound is indicated by the suffix "-ic".

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What does the suffix"ous" indicate in a chemical name?

The lower oxidation state of a metal in a compound is indicated by the suffix "-ous".

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What type of atoms form a covalent bond?

A covalent bond is formed between two nonmetal atoms.

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How are electrons shared in a covalent bond?

Covalent bonds occur when two atoms share electrons to achieve stability.

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What is a nonpolar covalent bond?

In a nonpolar covalent bond, the electrons are shared equally between the two atoms.

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Ionic compound

A compound formed by the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions).

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What is a polar covalent bond?

In a polar covalent bond, the electrons are not shared equally between the two atoms.

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What is electronegativity?

Electronegativity is the ability of an atom to attract electrons.

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Salt

A specific type of ionic compound where the positive ion is not hydrogen (H+) and the negative ion is not hydroxide (OH-)

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How is electronegativity used to determine the polarity of a covalent bond?

Electronegativity values are used to determine whether a covalent bond will be polar or nonpolar.

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Monatomic ion

An ion formed from a single atom that has gained or lost electrons.

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Metal cation

Positive ion formed by a metal atom losing electrons.

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Nonmetal anion

A negative ion formed by a nonmetal atom gaining electrons.

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Polyatomic ion

A group of covalently bonded atoms that carry a net charge.

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Polyatomic ion charge

The overall charge of a polyatomic ion applies to the entire group, not just the last element.

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Ternary ionic compound

A chemical compound formed by the electrostatic interaction between a metal cation and a polyatomic anion.

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Nonpolar Covalent Bond

A covalent bond where electrons are shared equally between two atoms with identical electronegativity values.

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Polar Covalent Bond

A covalent bond where electrons are shared unequally between two atoms with different electronegativity values.

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Structural Formula

A diagram that represents the arrangement of atoms in a molecule using lines to indicate covalent bonds.

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Lewis Dot Diagram (LDD)

A diagram that shows the arrangement of valence electrons around the atoms in a molecule.

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Diatomic Element

A type of molecule that contains only two atoms of the same element.

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Double Bond

A type of bond where two atoms share two pairs of electrons.

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Coordinate Covalent Bond

A bond where both electrons in the pair are donated by a single atom. One atom acts as a 'free-loader', contributing no electrons.

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Bond Energy

The energy required to break a bond between two atoms.

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Bond Length

The distance between the nuclei of two bonded atoms.

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Molecule-Ion attraction

A type of intermolecular force that occurs between polar molecules and ions.

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Intermolecular Forces (IMFs)

Attractive forces that exist between molecules. These forces are weaker than ionic or covalent bonds.

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Metallic Bonding

A special type of bonding that occurs only between metal atoms. In this type of bonding, metal atoms lose their valence electrons, forming positively charged ions. These electrons become delocalized, forming a 'sea' of electrons around the cations.

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Conductivity

The ability of a substance to conduct electricity. This is due to the presence of freely moving charged particles. For metals, these charged particles are electrons.

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Ionic Bond Conductivity

Solid ionic compounds do not conduct electricity because the ions are fixed within a crystal lattice. However, liquid or dissolved ionic compounds conduct electricity because the ions are free to move.

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Melting Point (mp)

The temperature at which a substance changes from a solid to a liquid.

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Boiling Point (bp)

The temperature at which a substance changes from a liquid to a gas.

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IMFs and Melting/Boiling Point

The stronger the attractive forces between molecules, the higher the boiling point and melting point of the substance.

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Study Notes

Bonding Unit

  • A chemical bond is an electrostatic attraction between the nuclei and valence electrons of different atoms.
  • Electrons are the subatomic particles involved in bonding.
  • Protons and neutrons are found in the nucleus.
  • Electrons are located outside the nucleus.
  • An orbital is the region where electrons are most likely to be found.
  • Valence shell is the outermost energy level.
  • Valence electrons are the electrons located in the valence shell.
  • Atoms with the same number of valence electrons behave similarly.
  • Atoms in the same group on the periodic table have the same number of valence electrons and therefore will bond/react similarly.
  • The maximum number of valence electrons is 8 (octet rule)
  • Atoms bond to become more stable.
  • An atom is stable when it has a full valence shell.
  • Noble gases/inert gases/group 18 are stable.

Types of Bonds

  • Ionic bonds form when electrons are transferred between atoms.
  • Covalent bonds form when electrons are shared between atoms.
  • Metallic bonds form when electrons are shared in a "sea" of freely moving electrons.
  • Ionic bonding exists in ionic compounds.
  • In ionic compounds the positive and negative ions combine in a ratio so the total number of positive charges equals the total number of negative charges.
  • Key terms for ionic : "Transfer of Electrons", "Salts", "Crystal Lattice Structures".
  • Metals lose electrons and nonmetals gain electrons.
  • The number of electrons lost by the metal(s) must equal the number of electrons gained by the nonmetal(s).
  • A binary compound is a compound composed of only two elements.
  • Ternary compounds are compounds that are composed of three or more elements.
  • Compounds are neutral.
  • Ions are charged particles.
  • Cations are positively charged ions
  • Anions are negatively charged ions
  • The electronegativity difference between the electronegativity values of the atoms within the compound determines covalent bond type.
  • A bond is considered ionic when the electronegativity difference is greater than or equal to 1.7.
  • The bigger the difference in electronegativity, the more polar the bond.
  • The smaller the difference in electronegativity, the less polar the bond.

Bond Formation

  • Energy is released when a bond is formed.
  • Energy is absorbed to break a bond.
  • Atoms bond to lower their potential energy.

Covalent Bonds

  • In covalent bonds electrons are shared between atoms
  • Covalent bonds generally form between nonmetals.
  • A covalent bond will have partial positive and negative charges if the electronegativity values of the atoms are not equal.
  • A covalent bond involves two or more atoms sharing electrons to fill their valence shells.
  • Nonpolar covalent bonds share electrons equally
  • Polar covalent bonds share electrons unequally.
  • Each type of covalent bond has a bond dissociation energy (strength) and a certain length.
  • A molecule with polar bonds will be polar only if its shape is asymmetrical and will not cancel out the dipoles that are present.
  • A molecule with polar bonds will be nonpolar only if its shape is symmetrical and the dipoles will cancel out.

Polyatomic Ions

  • Polyatomic ions are charged groups of covalently bonded atoms.
  • Polyatomic ions have a charge that applies to the entire group of atoms.
  • The names of polyatomic ions remain constant.
  • Keep the name that is on the table (table E).
  • When there is no number next to the charge, the number is really 1.
  • Ternary ionic compounds will always have one polyatomic ion and another monatomic ion or two polyatomic ions.

Naming Compounds

  • Use prefixes to indicate the number of atoms of each element.
  • Use the stock system (with roman numerals) if the metal can have more than one oxidation state.
  • Binary and ternary compounds have different naming conventions.

Intermolecular Forces

  • Intermolecular forces are the forces of attraction between molecules that exist between neighboring molecules.
  • There are three types of intermolecular forces:
  • Dispersion forces (or London dispersion forces): weak intermolecular forces that keep nonpolar molecules from being a gas at low temps.
  • Dipole-dipole forces: stronger than dispersion forces, occurring when the positive end of one dipole is attracted to the negative end of a nearby dipole.
  • Hydrogen bonds: strongest type of dipole-dipole attraction, where H is attracted to an electronegative atom (F, O, or N).
  • The stronger the intermolecular forces, the higher the boiling point.

Molecule Polarity

  • Molecule polarity is determined both by the polarity of the individual bonds and the molecular geometry.
  • If the dipoles cancel, the molecule is nonpolar.
  • If the dipoles do not cancel, the molecule is polar.
  • Like dissolves like (nonpolar dissolves nonpolar, polar dissolves polar, ionic dissolves polar).

Metallic Bonding

  • Metals have a "sea" of freely moving electrons.
  • Metals are excellent conductors in any phase because of free moving electrons.
  • Ionic solids do not conduct in a solid phase and do not conduct in the solid phase because of fixed ions.

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Test your knowledge on the fundamental concepts of chemical bonding. This quiz covers types of bonds, the role of electrons, and the periodic table's influence on bonding behavior. Perfect for students studying chemical interactions and bonding principles.

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