Intermolecular Forces and Compounds

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Questions and Answers

Which of the following elements is NOT involved in the formation of calcium oxide?

  • Chlorine (correct)
  • Sodium (correct)
  • Oxygen
  • Calcium

Ionic bonds are formed when two atoms share electrons.

False (B)

What is the primary difference between ionic and covalent bonds?

Ionic bonds involve the transfer of electrons between atoms, leading to the formation of ions, while covalent bonds involve the sharing of electrons between atoms.

The high melting point of common salt is due to the strong ______ forces between the ions.

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

Match the following terms with their definitions:

<p>Cation = An atom that has gained electrons Anion = An atom that has lost electrons Covalent bond = A chemical bond formed by the sharing of electrons between two atoms Ionic bond = A chemical bond formed by the electrostatic attraction between oppositely charged ions</p> Signup and view all the answers

Which of the following solutions will allow electricity to conduct?

<p>Copper sulphate solution (A), Salt solution (B)</p> Signup and view all the answers

Sugar solutions can conduct electricity like ionic compounds.

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

What type of bond do common salt and copper sulphate contain?

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

In its _____ state, common salt can also conduct electricity.

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

What was used in the experiment to test for electrical conductivity?

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

How does electricity flow through ionic compounds?

<p>In aqueous solution and fused state.</p> Signup and view all the answers

Match the compounds with their type:

<p>Common salt = Ionic compound Sugar = Covalent compound Copper sulphate = Ionic compound Distilled water = Covalent compound</p> Signup and view all the answers

Electricity flows through solid ionic compounds.

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

Which type of compounds typically have high melting points and boiling points?

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

Covalent compounds conduct electricity in aqueous solutions.

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

What is the typical state of ionic compounds at room temperature?

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

The melting point of sodium chloride is _____ °C.

<p>801</p> Signup and view all the answers

Which of the following statements is true regarding covalent compounds?

<p>Most are liquids or gases at room temperature. (A)</p> Signup and view all the answers

Match the following compounds with their bond type:

<p>Sodium chloride = Ionic Water = Covalent Calcium oxide = Ionic Ammonia = Covalent</p> Signup and view all the answers

Ionic compounds are generally soluble in water.

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

Oxygen has a melting point of _____ °C.

<p>-218</p> Signup and view all the answers

What type of bonds are responsible for the special properties of water?

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

Intermolecular forces are stronger than covalent bonds in a water molecule.

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

What state would water be in at room temperature if there were no intermolecular forces?

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

Water has special properties due to ___________ forces among its molecules.

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

Match the following types of bonds with their characteristics:

<p>Covalent bonds = Strong bonds formed by shared electrons Intermolecular bonds = Weaker bonds between molecules Ionic bonds = Formed between charged ions Metallic bonds = Bonds between metal atoms with free electrons</p> Signup and view all the answers

Which of the following is NOT a property of water explained by intermolecular forces?

<p>High melting point (C)</p> Signup and view all the answers

Intermolecular bonds allow water to exist as a liquid at room temperature.

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

What forces are responsible for water's behavior and unique physical properties?

<p>Intermolecular forces</p> Signup and view all the answers

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Flashcards

Intermolecular Bonds

Forces of attraction between molecules rather than within them.

Covalent Bonds

Stronger bonds formed by sharing electrons between atoms.

Water's Liquid State

Water remains liquid at room temperature due to intermolecular forces.

Water as a Gas

Without intermolecular forces, water turns into gas at room temperature.

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Special Properties of Water

Properties such as high surface tension and boiling point due to intermolecular forces.

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Oxygen Atom in Water

Oxygen atom in water is partially negative, attracting hydrogen atoms.

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Hydrogen Atoms in Water

Hydrogen atoms in water are partially positive, forming bonds with oxygen.

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Attractive Forces

Forces that hold water molecules together, influencing its properties.

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High Boiling Point

The temperature at which a substance turns from liquid to gas is high for water due to hydrogen bonding.

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High Specific Heat Capacity

The amount of heat required to raise the temperature of a substance significantly is notably high for water.

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Density of Ice

Ice is less dense than liquid water, which is why it floats.

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Ionic Compounds

Compounds made of ions that conduct electricity when dissolved in water or molten.

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Covalent Compounds

Compounds formed by shared electrons that do not conduct electricity in solution.

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Conductivity Test

An experiment to measure how well a solution conducts electricity.

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Fused Ionic Compounds

Ionic compounds that conduct electricity when melted.

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Solid Ionic Compounds

In solid-state, ionic compounds do not conduct electricity because ions are fixed in place.

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Ionic compound characteristics

Ionic compounds consist of oppositely charged ions, are solid at room temperature, have high melting/boiling points, conduct electricity in molten or aqueous states, and are mostly soluble in water.

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Covalent compound characteristics

Covalent compounds are made of molecules, generally exist as gases or liquids, have low melting/boiling points, do not conduct electricity in aqueous solutions, and some are soluble in water.

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Melting point of sodium chloride

The melting point of sodium chloride is 801°C.

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Boiling point of water

Water has a boiling point of 100°C.

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Conductivity in ionic compounds

Ionic compounds can conduct electricity when they are molten or dissolved in water.

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Conductivity in covalent compounds

Covalent compounds generally do not conduct electricity in aqueous solutions.

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Examples of ionic compounds

Sodium chloride and calcium oxide are examples of ionic compounds.

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Examples of covalent compounds

Water and ammonia are examples of covalent compounds.

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Ion

An atom or molecule with a net electrical charge due to loss or gain of electrons.

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Cation

A positively charged ion, formed by the loss of one or more electrons.

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Anion

A negatively charged ion, formed by gaining one or more electrons.

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Ionic Bond

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

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Polarity

A property of molecules having a difference in electrical charge, leading to positive and negative ends.

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Hydrogen Bond

A weak attraction between a hydrogen atom and an electronegative atom, such as oxygen.

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Intermolecular Forces

Forces of attraction or repulsion between neighboring molecules, affecting properties like boiling point.

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Study Notes

Intermolecular Forces in Water

  • Intermolecular forces in water are weaker than covalent bonds within a water molecule.
  • These forces give water special properties at room temperature, like being a liquid instead of a gas.
  • Water's high boiling point, high specific heat capacity, and higher density than ice are all due to attractive forces between water molecules.

Properties of Ionic and Covalent Compounds

  • Ionic compounds (like common salt and copper sulfate) conduct electricity in solutions or when melted.
  • Covalent compounds (like sugar and water) do not conduct electricity in solutions or as solids.
  • Ionic compounds are typically solids at room temperature with high melting and boiling points.
  • Covalent compounds are typically liquids or gases at room temperature with lower melting and boiling points.

Melting and Boiling Points of Compounds

  • Ionic compounds typically have very high melting and boiling points (NaCl, 801/1413 °C).
  • Covalent compounds, on the other hand, often have low melting and boiling points (many are fluids at room temp).
  • Water (Hâ‚‚O) being a covalent compound, has a relatively high boiling point of 100°C.
  • This high boiling point, despite it being a covalent compound, is due to the strong intermolecular forces (hydrogen bonding) within water molecules.

Characteristics of Ionic Compounds

  • Ionic compounds are formed from oppositely charged ions (+ and -).
  • These compounds typically form solid crystalline structures at room temperature.
  • They have high melting points and boiling points.
  • They conduct electricity in liquid or dissolved states.
  • They are often soluble in water.

Characteristics of Covalent Compounds

  • Covalent compounds exist mainly as molecules comprised of multiple atoms.
  • Most covalent compounds are liquids or gases at room temperature
  • They often have low melting points and boiling points.
  • Their aqueous (dissolved in water) solutions typically do not conduct electricity.
  • Some covalent compounds are soluble in water.

Summary of Compound Formation

  • Compounds form when atoms of different elements chemically bond.
  • During bonding, electrons in atoms' valence shells rearrange.
  • Positive ions (cations) form when atoms lose electrons, while negative ions (anions) form when atoms gain electrons.
  • Electrostatic forces between oppositely charged ions create ionic bonds.
  • Sharing electrons forms covalent bonds.
  • The structure of ionic compounds forms a crystalline lattice arrangement of ions.
  • Covalent compounds form discrete molecules.
  • Intermolecular forces affect the properties of compounds.

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