Covalent and Ionic Bonds
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Questions and Answers

Which statement accurately describes the behavior of atoms in a covalent bond?

  • Atoms transfer electrons to achieve a stable electron configuration.
  • Atoms gain electrons to achieve a stable electron configuration.
  • Atoms share electrons to achieve a stable electron configuration. (correct)
  • Atoms lose electrons to achieve a stable electron configuration.

Which of the following molecules contains a double covalent bond?

  • CH4
  • HCl
  • NH3
  • O2 (correct)

Why do ionic compounds typically exhibit high melting and boiling points?

  • The covalent bonds within the ions require significant energy to break.
  • Weak Van der Waals forces exist between the ions.
  • Strong electrostatic forces of attraction between oppositely charged ions require a lot of energy to overcome. (correct)
  • The kinetic energy of the ions is minimal, preventing easy separation.

How many shared electrons are present in a triple covalent bond?

<p>6 (B)</p> Signup and view all the answers

Under what conditions can ionic compounds conduct electricity?

<p>When molten or dissolved in water, allowing ions to move freely and carry charge. (A)</p> Signup and view all the answers

In a molecule of nitrogen gas (N2), how many lone pairs of electrons are present in total?

<p>4 (B)</p> Signup and view all the answers

Which statement accurately describes the arrangement of ions in an ionic compound?

<p>Oppositely charged ions arrange themselves into a repeating pattern called a lattice. (C)</p> Signup and view all the answers

Which of the following molecules contains only single covalent bonds?

<p>H2O (C)</p> Signup and view all the answers

Carbon dioxide (CO2) contains how many double bonds?

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

Why are ionic crystals considered brittle?

<p>The strong repulsive forces between ions of the same charge cause the crystal to shatter when stressed. (C)</p> Signup and view all the answers

Why don't ionic compounds conduct electricity in the solid-state?

<p>The ions are locked in place and cannot move to carry a charge. (B)</p> Signup and view all the answers

What is the primary force of attraction that holds atoms together in a covalent bond?

<p>The attraction between the nuclei and shared electrons. (C)</p> Signup and view all the answers

What type of elements are typically involved in covalent bonding?

<p>Usually only non-metal elements. (B)</p> Signup and view all the answers

Methane (CH4) is a simple molecular structure. What type of bonds does carbon form with hydrogen in methane?

<p>Single covalent bonds (D)</p> Signup and view all the answers

What process occurs when ionic compounds dissolve in water that allows them to conduct electricity?

<p>The ions dissociate and are free to move, carrying electrical current. (A)</p> Signup and view all the answers

What is the main principle behind the formation of a covalent bond?

<p>Sharing electrons between atoms to achieve a stable electron configuration. (B)</p> Signup and view all the answers

Which of the following statements accurately describes the process of ionic bond formation?

<p>Atoms transfer electrons, resulting in the formation of oppositely charged ions that are attracted to each other. (A)</p> Signup and view all the answers

What is the formula of the ionic compound formed between Aluminum (Al), which is in group 3, and Oxygen (O), which is in group 6?

<p>Al2O3 (D)</p> Signup and view all the answers

Which of the following is the correct dot-and-cross diagram representation for the formation of sodium chloride (NaCl) from its elements?

<p>Na+[x] [Cl[o o o o o o]]- (C)</p> Signup and view all the answers

Which of these polyatomic ions has a positive charge?

<p>NH4+ (D)</p> Signup and view all the answers

Consider the formation of an ionic compound between a Group 2 element and a Group 7 element. Which of the following statements is correct regarding the electron transfer?

<p>The Group 2 element loses two electrons, and two Group 7 elements each gain one electron. (C)</p> Signup and view all the answers

Which of the following is NOT a typical property of ionic compounds?

<p>Low solubility in polar solvents (C)</p> Signup and view all the answers

An element from which group would most likely form an ionic bond with an element from Group 6?

<p>Group 1 (C)</p> Signup and view all the answers

Which of the following describes what happens when magnesium reacts with oxygen to form magnesium oxide?

<p>Magnesium loses two electrons to oxygen, forming Mg2+ and O2- ions, resulting in an ionic bond. (B)</p> Signup and view all the answers

What primarily determines the melting and boiling points of simple molecular structures like fullerenes?

<p>The strength of the intermolecular forces between molecules. (D)</p> Signup and view all the answers

Why do molecules with higher formula mass generally have higher melting and boiling points?

<p>Larger molecules exhibit stronger intermolecular forces that demand more energy to overcome. (B)</p> Signup and view all the answers

What happens to covalent bonds when water boils?

<p>Covalent bonds are unaffected. (A)</p> Signup and view all the answers

Which property of graphite is a direct result of its delocalized electrons?

<p>Its ability to conduct electricity. (A)</p> Signup and view all the answers

Why does diamond have a significantly higher melting point than C60 fullerene?

<p>Diamond is a giant covalent structure, requiring the breaking of covalent bonds to melt, whereas C60 fullerene is a simple molecular structure. (B)</p> Signup and view all the answers

What structural feature of graphite allows its layers to slide easily over each other, making it useful as a lubricant?

<p>Each carbon atom forms three covalent bonds, resulting in a layered structure. (A)</p> Signup and view all the answers

Based on the provided data, predict which halogen would have the lowest boiling point:

<p>Fluorine (F2) (D)</p> Signup and view all the answers

Which of the following best explains why diamond is extremely hard while graphite is relatively soft?

<p>Diamond has a three-dimensional network of strong covalent bonds, while graphite has layers held together by weaker forces. (D)</p> Signup and view all the answers

Which characteristic is typical of substances with simple molecular structures?

<p>Low boiling points due to weak intermolecular forces. (D)</p> Signup and view all the answers

Which type of bonding is primarily responsible for the high melting point in giant covalent structures?

<p>Strong covalent bonds throughout the structure. (C)</p> Signup and view all the answers

Why don't covalent molecular compounds conduct electricity?

<p>Their electrons are tightly held within atoms or covalent bonds. (B)</p> Signup and view all the answers

How does increasing molecular mass generally affect the boiling point of simple molecular substances?

<p>Increases the boiling point due to stronger intermolecular forces. (D)</p> Signup and view all the answers

Which allotrope of carbon conducts electricity?

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

Which of the following substances is held together by weak intermolecular forces?

<p>Hydrogen ($H_2$) (D)</p> Signup and view all the answers

A substance is found to have a melting point of 300°C and does not conduct electricity in solid or liquid form. Based on this information, which type of structure is most likely?

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

Why does diamond have a very high melting point?

<p>A high amount of energy is needed to break the strong covalent bonds between carbon atoms in its 3D tetrahedral structure. (A)</p> Signup and view all the answers

Graphite conducts electricity, whereas diamond does not. What is the primary reason for this difference?

<p>Each carbon atom in graphite bonds with only three others, leaving its fourth outer electron free to move through the layers. (D)</p> Signup and view all the answers

A scientist is studying a new carbon-based material. It is insoluble in water but soluble in organic solvents. Based on this information, what type of bonding is most likely present in this material?

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

How does the number of bonds formed by each carbon atom differ between diamond and graphite, and what impact does this difference have on their properties?

<p>Diamond forms four bonds per carbon atom, contributing to its hardness and lack of electrical conductivity, while graphite forms three, allowing for electrical conductivity. (A)</p> Signup and view all the answers

Consider two carbon allotropes: one that is extremely hard and does not conduct electricity, and another that is soft and conducts electricity. Which of the following statements accurately identifies the two?

<p>Diamond is hard and non-conductive, while graphite is soft and conductive. (A)</p> Signup and view all the answers

Flashcards

Ionic Bonding

The transfer of electrons from one atom to another, creating ions that are then attracted to each other.

Dot-and-Cross Diagrams (Ionic)

A visual representation showing the transfer of electrons in ionic bonding, using dots and crosses to distinguish electron origins.

Ions

Atoms or molecules that have gained or lost electrons, resulting in a net electrical charge

Cation

A positively charged ion formed when an atom loses electrons.

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Anion

A negatively charged ion formed when an atom gains electrons.

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Ionic Bond

The electrostatic force of attraction between oppositely charged ions.

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Covalent Bond

Atoms share electrons to achieve a full outer shell.

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Dot-and-Cross Diagrams (Covalent)

Diagrams that show the arrangement of electrons within a molecule and how electrons are shared (covalent)

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Molecule

A substance formed when atoms are held together by covalent bonds.

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Lone Pairs

Pairs of electrons that are not involved in bonding.

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Single Covalent Bond

A bond where one pair of electrons is shared between two atoms.

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Double Covalent Bond

A bond where two pairs of electrons are shared between two atoms.

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Triple Covalent Bond

A bond where three pairs of electrons are shared between two atoms.

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Simple Molecular Structures

Molecules made up of only a few atoms.

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Covalent Bond Attraction

The attraction between the positively charged nuclei and the negatively charged shared electrons.

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Electrostatic Attraction (Ionic)

Strong attraction between oppositely charged ions.

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Giant Ionic Lattice

Repeating pattern of alternating charges in ionic compounds, where each ion is surrounded by ions of the opposite charge.

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Melting/Boiling Point of Ionic Compounds

High due to strong electrostatic forces, requiring much energy to break the bonds.

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Solubility of Ionic Compounds

Usually soluble in water, insoluble in organic solvents.

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Electrical Conductivity of Ionic Compounds

Do not conduct electricity as solids, but conduct when molten or dissolved because ions are free to move.

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Movement of Ions

Ions are fixed in place. They cannot move to carry electrical current. Instead, the ions are moving when ionic compounds are molten or dissolved.

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Shape of Ionic Compounds

Crystalline structures due to repeating arrangement of ions.

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Covalent Solubility

Most covalent substances do not dissolve in water but do dissolve in organic solvents.

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Diamond: Bonds per Carbon

Each Carbon atom is bonded to four other carbon atoms.

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Diamond's Conductivity

Does not conduct electricity because all outer shell electrons are held in covalent bonds, leaving no free electrons to move.

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Graphite's Conductivity

Each carbon atom bonds with only 3 others, leaving one electron free to move throughout the layers. These are called delocalised electrons.

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Graphite: Bonds per Carbon

Each carbon atom is bonded to three other carbon atoms in layers.

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Intermolecular Forces

Weak forces that hold molecules together. Much weaker than covalent bonds.

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Giant Covalent Structures

Held together by strong covalent bonds; high melting and boiling points.

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Allotrope

A substance that consists of only one type of atom.

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Diamond Structure

Each carbon atom forms 4 covalent bonds in a 3D tetrahedral structure, making it extremely hard with a high melting point.

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Graphite Structure

Each carbon atom forms 3 covalent bonds in 2D sheets that can slide. Contains delocalized electrons that conduct electricity.

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Molecule Definition

A fixed number of atoms joined by covalent bonds.

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Intermolecular Forces

The forces of attraction between molecules.

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Delocalized Electrons

Electrons not involved in bonding that are free to move and conduct electricity.

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Melting/Boiling Point of Simple Molecules

Low melting and boiling points due to weak intermolecular forces.

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Fullerene (C60)

A simple molecular structure with a fixed number of atoms, held together by weak intermolecular forces.

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Electrical Conductivity of Covalent Molecular Compounds

Do not conduct electricity because electrons are tightly held.

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High Melting Points in Giant Structures

Breaking covalent bonds requires a lot of energy, leading to very high melting points.

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Formula Mass and Boiling Point

Molecules with larger formula mass have stronger intermolecular forces, thus higher melting/boiling points.

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Boiling Point vs. Molecular Mass

Boiling point increases with higher molecular mass.

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Study Notes

  • Review of ionic and covalent bonding concepts.
  • How to represent ionic compounds and molecules diagrams.
  • Overview of properties for each type of compound.
  • Exploration of the structures in diamond, and in graphite.
  • Textbook reference: ionic (pages 75-83), covalent (pages 85-96).

Ionic Bonding

  • Involves electron transfer.
  • Groups 1, 2, and 3 atoms lose electrons to achieve a full outer shell.
  • Groups 5, 6, and 7 atoms gain electrons to achieve a full outer shell.
  • An ion refers to an atom or molecule possessing a net electric charge due to the loss or gain of one or more electrons.
  • Sodium gives away one outer electron to chlorine to form an ionic bond: sodium chloride.
  • The resulting positive and negative charges attract each other.

Dot-and-Cross Diagrams

  • Illustrate electron behavior during compound formation.
  • The first step is to draw the original atoms.
  • The second step is to indicate electron transfer using arrows.
  • The third is to represent the ions that are formed.
  • For the third step, ions are drawn with the full outer shell, enclosed in square brackets, and showing the charge in the top right corner.

Ionic Bonds

  • Formation from electrostatic attraction: a strong attraction force exists between oppositely charged ions.
  • Ions arrange into a giant ionic lattice: creating a repeating pattern of alternating charges due to electrostatic forces.
  • This arrangement ensures each ion is surrounded by ions possessing the opposite charge.
  • This arrangement leads to a "lattice" structure:.

Properties of Ionic Compounds

  • Exhibit high melting and boiling points: this requires a significant amount of energy to overcome the lattice's attraction forces.
  • Crystalline shape: can assume crystalline shapes such as when ionic compounds form crystals under microscopes.
  • Tend to be brittle.
  • Tend to be soluble in water but insoluble in organic solvents like ethanol or acetone.
  • Do not conduct electricity as solids: ions are fixed in place.
  • Conduct electricity when molten or dissolved in water: ions are free to move.

Covalent Bonding

  • Occurs when atoms share electrons to complete their octet.
  • Typically involves non-metal elements.
  • Resulting substance referred to as a molecule.
  • A covalent bond forms when atoms share electrons equally.
  • Fluorine (group 7) with 7 outer electrons, needs one more to fill the outer shell; will bond covalently.
  • In a covalent bond, a pair of shared electrons is known as a single covalent bond.
  • Single covalent bond: a total of 8 electrons per atom, follows octet rule, and can be represented with a line.
  • Oxygen (group 6) can form two types of bonds: two single bonds or one double bond.
  • Nitrogen (group 5) can form two types of bonds: three single bonds or one triple bond.
  • Single Bond: contains 1 bond which means there are 2 shared electrons which equals 1 pair.
  • Double Bond: contains 2 bonds which means there are 4 shared electrons which equals 2 pairs.
  • Triple Bond: contains 3 bonds which means there are 6 shared electrons which equals 3 pairs.
  • Carbon (group 4) typically forms 4 bonds.

Covalent Bonding

  • Atoms join together due to the nuclei attracting the shared electrons.
  • Molecules held together by covalent bonds (strong) and intermolecular forces (weak).
  • Simple molecular structures: formed by molecules with few atoms where attraction from covalent bonds is strong.
  • Intermolecular forces between molecules are weak: the weak forces that are broken when water boils.
  • A few elements and compounds with covalent bonding include: water (H2O), methane (CH4), carbon dioxide (CO2), ammonia (NH3), hydrochloric acid (HCl), and diatomic oxygen (O2).

Halogens

  • Molecules with higher formula mass exhibit higher melting and boiling points.
  • More energy is needed to break the intermolecular forces.
  • Examples of halogens: Fluorine (F2), Chlorine (Cl2), Bromine (Br2), and Iodine (I2).

Giant Covalent Structures

  • Very large structures of atoms with no fixed number of atoms.
  • Each carbon in diamond bonds to four others: creating a strong 3D tetrahedral shape which is extremely strong.
  • Very high melting point (almost 4000°C) is required to break the covalent bonds.
  • Each carbon in graphite only forms 3 bonds.
  • Carbon atoms arrange in 2D sheets that slide: making graphite softer than diamond and easily broken.
  • Unbonded electron forms delocalized electron: this allows graphite to conduct electricity.
  • High melting point from giant covalent structure.
  • C60 Fullerene is a simple molecular structure: fixed number of atoms and low melting/boiling point.
  • Only weak intermolecular forces hold molecules together.

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Lesson PDF: Review of Ionic and Covalent Bonding PDF

Description

Explore covalent and ionic bonds in chemistry. Learn about electron sharing, attraction forces, and the differences in conductivity between these bond types. These questions cover key aspects of chemical bonding.

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