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A double bond consists of one sigma bond and two pi bonds.
A double bond consists of one sigma bond and two pi bonds.
False
Ionic compounds usually have high melting and boiling points.
Ionic compounds usually have high melting and boiling points.
True
Covalent compounds generally conduct electricity when dissolved in water.
Covalent compounds generally conduct electricity when dissolved in water.
False
The Valence Shell Electron Pair Repulsion Theory (VSEPR Theory) determines the shapes of ionic compounds.
The Valence Shell Electron Pair Repulsion Theory (VSEPR Theory) determines the shapes of ionic compounds.
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In a nitrogen molecule, two 2px orbitals overlap head-on to form a sigma bond.
In a nitrogen molecule, two 2px orbitals overlap head-on to form a sigma bond.
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Transition metals can form ions with different charges.
Transition metals can form ions with different charges.
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Zinc is considered a transition metal.
Zinc is considered a transition metal.
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Covalent bonding involves the transfer of electrons between atoms.
Covalent bonding involves the transfer of electrons between atoms.
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A hydrogen molecule is formed by the sharing of one electron from each hydrogen atom.
A hydrogen molecule is formed by the sharing of one electron from each hydrogen atom.
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An oxygen atom needs to share four electrons to complete its octet.
An oxygen atom needs to share four electrons to complete its octet.
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A sigma bond can be formed by sideways overlap of orbitals.
A sigma bond can be formed by sideways overlap of orbitals.
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The valency of chlorine is two.
The valency of chlorine is two.
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Manganese can form ions with a charge of +7.
Manganese can form ions with a charge of +7.
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The formula for Sodium Sulfate is NaSO4.
The formula for Sodium Sulfate is NaSO4.
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Hydrogencarbonate ion has a charge of -2.
Hydrogencarbonate ion has a charge of -2.
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Iron (II) Chloride is represented by FeCl3.
Iron (II) Chloride is represented by FeCl3.
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The formula for Calcium Hydrogencarbonate is Ca(HCO3)2.
The formula for Calcium Hydrogencarbonate is Ca(HCO3)2.
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Transition metals generally exhibit variable valency due to small energy differences between 4s and 3d orbitals.
Transition metals generally exhibit variable valency due to small energy differences between 4s and 3d orbitals.
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The formula for Iron (II) carbonate is Fe(CO3)2.
The formula for Iron (II) carbonate is Fe(CO3)2.
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The Phosphate ion has a charge of -2.
The Phosphate ion has a charge of -2.
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Copper (II) oxide is represented by CuO.
Copper (II) oxide is represented by CuO.
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Water is a non-polar liquid as it does not exhibit attraction to charged objects.
Water is a non-polar liquid as it does not exhibit attraction to charged objects.
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An electronegativity difference greater than 1.7 indicates ionic bonding in a compound.
An electronegativity difference greater than 1.7 indicates ionic bonding in a compound.
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A covalent bond is classified as non-polar if the E.N difference is less than or equal to 0.4.
A covalent bond is classified as non-polar if the E.N difference is less than or equal to 0.4.
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Sodium chloride dissolves in water due to the strong attraction between water molecules and the ions of sodium chloride.
Sodium chloride dissolves in water due to the strong attraction between water molecules and the ions of sodium chloride.
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If a liquid shows attraction when a charged rod is brought near, it is classified as non-polar.
If a liquid shows attraction when a charged rod is brought near, it is classified as non-polar.
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The molecule CH4 has a significant electronegativity difference, implying it is a polar molecule.
The molecule CH4 has a significant electronegativity difference, implying it is a polar molecule.
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Intramolecular bonding occurs between different molecules.
Intramolecular bonding occurs between different molecules.
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A polar covalent bond has an electronegativity difference greater than 0.4 but less than 1.7.
A polar covalent bond has an electronegativity difference greater than 0.4 but less than 1.7.
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PH3 is considered a polar covalent compound.
PH3 is considered a polar covalent compound.
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Hydrogen bonding occurs in both H2O and NH3 but not in PH3.
Hydrogen bonding occurs in both H2O and NH3 but not in PH3.
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The shape of the PH3 molecule is linear according to electron-pair repulsion theory.
The shape of the PH3 molecule is linear according to electron-pair repulsion theory.
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Boron trichloride (BCl3) is a polar molecule due to its asymmetrical shape.
Boron trichloride (BCl3) is a polar molecule due to its asymmetrical shape.
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Water is a polar solvent primarily due to the electron configuration of hydrogen.
Water is a polar solvent primarily due to the electron configuration of hydrogen.
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Hydrogen bonding is the weakest form of intermolecular force.
Hydrogen bonding is the weakest form of intermolecular force.
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The bond angle in ammonia is 109.5°.
The bond angle in ammonia is 109.5°.
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Iodine is a pure polar molecule.
Iodine is a pure polar molecule.
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A molecule with polar bonds can still be non-polar.
A molecule with polar bonds can still be non-polar.
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Ammonia exhibits hydrogen bonding due to the presence of a highly electronegative element.
Ammonia exhibits hydrogen bonding due to the presence of a highly electronegative element.
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The shape of a molecule with the formula QX4 is linear.
The shape of a molecule with the formula QX4 is linear.
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The electronegativity difference is greater for the Si–H bond than for the N–H bond.
The electronegativity difference is greater for the Si–H bond than for the N–H bond.
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Hydrogen has stronger intermolecular forces than oxygen at low temperatures.
Hydrogen has stronger intermolecular forces than oxygen at low temperatures.
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Study Notes
Chemical Bonding
- A compound is a substance made of two or more different elements combined chemically.
- Chemical bonds hold atoms together in a compound.
- The octet rule states atoms tend to gain, lose, or share electrons to achieve eight electrons in their outermost energy level (stable).
- Some elements (transition metals, hydrogen, lithium, and beryllium) do not follow the octet rule.
- An ion is a charged atom or group of atoms.
- Atoms form ions by gaining or losing electrons to achieve a noble gas configuration.
- Ionic bonding involves the complete transfer of electrons from one atom to another, forming oppositely charged ions that attract each other.
- Ionic compounds have high melting and boiling points, are usually solids at room temperature, hard and brittle, and conduct electricity when molten or dissolved in water.
- Formulae represent compounds’ elements and how many of each.
- Ionic compounds are formed between metals (groups I and II) and non-metals (groups VI and VII).
- A crystal lattice is a three-dimensional arrangement of ions.
Ionic Compounds - Formulas
- Elements in groups I and II tend to lose electrons to form positively charged ions (cations).
- Elements in groups VI and VII tend to gain electrons to form negatively charged ions (anions).
- Ionic compounds are overall neutral; thus, positive and negative charges must balance.
- The formula for any ionic compound is determined by ensuring the total positive charge equals the total negative charge.
Dot and Cross Diagrams
- Show the outer electrons of each atom.
- Represent atoms with dots or crosses (different symbols).
- Use an arrow to show electron transfer.
How to Write the Formulas of Ionic Compounds
- Represent atoms using symbols.
- Use numbers to show the number of atoms of each element.
- For Ionic compounds, determine the formulas by ensuring the total positive charge equals the negative charge.
Covalent Bonding
- Covalent bonds involve the sharing of electrons between atoms.
- Atoms share electrons to achieve a stable electron configuration.
- Molecules are groups of atoms joined together. The smallest particle of an element or compound.
- A sigma bond occurs when atomic orbitals overlap head-on.
- A pi bond occurs when p orbitals overlap sideways.
Types of bonds
- Single bonds consist of one sigma bond.
- Double bonds consist of one sigma and one pi bond.
- Triple bonds consist of one sigma and two pi bonds.
- Polar Covalent bond: Unequal sharing of electrons.
- Non-polar Covalent bond: Equal sharing of electrons.
- Electronegativity is the measure of an atom's attraction for shared electrons in a covalent bond.
Properties of Covalent Compounds
- Often soft solids, liquids, or gases at room temperature.
- Have low melting and boiling points.
- Do not conduct electricity, either as solids or in solution.
Shapes of Covalent Molecules
- VSEPR Theory (Valence Shell Electron Pair Repulsion) predicts the shape of molecules based on electron pair repulsion.
- The shape of a molecule depends on the number of bond pairs and lone pairs around the central atom.
Electronegativity
- Electronegativity is the relative attraction of an atom for the shared pair of electrons in a covalent bond.
- The electronegativity difference between two atoms determines if the bond is polar.
- Polar Bonds- When the electronegativity difference between atoms in a molecule is greater than 0.4 but less than 1.7.
- Non-polar Bonds- When electronegativity difference between atoms is less than or equal to 0.4.
- Ionic Bonds- When electronegativity difference is greater than 1.7.
Intermolecular Forces
- Intermolecular forces are forces between molecules.
- Van der Waals forces are weak attractive forces between non-polar molecules resulting from temporary dipoles.
- Dipole-dipole forces exist between polar molecules.
- Hydrogen bonding is a strong type of dipole-dipole attraction between molecules with hydrogen bonded to a highly electronegative element (N, O or F).
Differences between ionic and covalent compounds
- Ionic compounds have high melting and boiling points; covalent compounds have low melting and boiling points.
- Ionic compounds are usually hard and brittle; covalent compounds are usually soft and flexible or gases.
- Ionic compounds can conduct electricity in their molten or dissolved states; covalent compounds do not conduct electricity.
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Description
Test your knowledge on chemical bonding concepts. This quiz covers topics such as compounds, chemical bonds, the octet rule, ionic bonding, and the properties of ionic compounds. Challenge yourself to understand how atoms interact to form stable structures!
