Podcast
Questions and Answers
Sodium Chloride has a ______ structure.
Sodium Chloride has a ______ structure.
cubic
Each sodium ion is surrounded by ______ chloride ions.
Each sodium ion is surrounded by ______ chloride ions.
6
Metals tend to ______ electrons while non-metals tend to gain electrons.
Metals tend to ______ electrons while non-metals tend to gain electrons.
lose
An ionic compound must have the same number of positive and ______ charges.
An ionic compound must have the same number of positive and ______ charges.
Signup and view all the answers
The formula for Aluminium Oxide is ______.
The formula for Aluminium Oxide is ______.
Signup and view all the answers
A compound is a substance made up of two or more different elements combined together ______.
A compound is a substance made up of two or more different elements combined together ______.
Signup and view all the answers
The forces that hold the atoms together in a new substance are called ______ bonds.
The forces that hold the atoms together in a new substance are called ______ bonds.
Signup and view all the answers
According to the Octet Rule, atoms tend to reach an electron arrangement with ______ electrons in the outermost energy level.
According to the Octet Rule, atoms tend to reach an electron arrangement with ______ electrons in the outermost energy level.
Signup and view all the answers
Noble gases are considered ______ because they have stable electron configurations.
Noble gases are considered ______ because they have stable electron configurations.
Signup and view all the answers
An ion is a ______ atom or group of atoms.
An ion is a ______ atom or group of atoms.
Signup and view all the answers
A negative ion is called an ______.
A negative ion is called an ______.
Signup and view all the answers
An ionic bond is the force of attraction between ______ charged ions in a compound.
An ionic bond is the force of attraction between ______ charged ions in a compound.
Signup and view all the answers
The outer electrons of one atom in a dot and cross diagram are represented by ______.
The outer electrons of one atom in a dot and cross diagram are represented by ______.
Signup and view all the answers
A double bond consists of one sigma bond and one ______ bond.
A double bond consists of one sigma bond and one ______ bond.
Signup and view all the answers
The two 2px orbitals in a nitrogen molecule overlap head-on to form a ______ bond.
The two 2px orbitals in a nitrogen molecule overlap head-on to form a ______ bond.
Signup and view all the answers
Ionic compounds usually exhibit ______ melting and boiling points.
Ionic compounds usually exhibit ______ melting and boiling points.
Signup and view all the answers
The Valence Shell Electron Pair Repulsion Theory is also known as ______ Theory.
The Valence Shell Electron Pair Repulsion Theory is also known as ______ Theory.
Signup and view all the answers
Covalent compounds do not conduct electricity when ______ in water.
Covalent compounds do not conduct electricity when ______ in water.
Signup and view all the answers
Transition metals are found in the ______, except for Scandium and Zinc.
Transition metals are found in the ______, except for Scandium and Zinc.
Signup and view all the answers
A transition metal forms at least one ion with a partially filled ______ sub-level.
A transition metal forms at least one ion with a partially filled ______ sub-level.
Signup and view all the answers
Manganese can form ions with a charge of +2, +4, or +______.
Manganese can form ions with a charge of +2, +4, or +______.
Signup and view all the answers
Covalent bonding involves electrons being ______ between atoms.
Covalent bonding involves electrons being ______ between atoms.
Signup and view all the answers
A chlorine atom needs to create a stable octet by ______ electrons with another chlorine atom.
A chlorine atom needs to create a stable octet by ______ electrons with another chlorine atom.
Signup and view all the answers
The electrons not involved in bonding are called ______ pairs.
The electrons not involved in bonding are called ______ pairs.
Signup and view all the answers
A ______ bond is formed by the head-on overlap of two orbitals.
A ______ bond is formed by the head-on overlap of two orbitals.
Signup and view all the answers
Since oxygen combines with two atoms of hydrogen, it has a valency of ______.
Since oxygen combines with two atoms of hydrogen, it has a valency of ______.
Signup and view all the answers
The method for using the VSEPR Theory includes drawing a dot and cross diagram of the ______.
The method for using the VSEPR Theory includes drawing a dot and cross diagram of the ______.
Signup and view all the answers
In VSEPR Theory, the shape of a molecule is determined using the number of bond pairs and ______ pairs.
In VSEPR Theory, the shape of a molecule is determined using the number of bond pairs and ______ pairs.
Signup and view all the answers
A molecule with 3 bond pairs and 0 lone pairs is categorized as ______ planar.
A molecule with 3 bond pairs and 0 lone pairs is categorized as ______ planar.
Signup and view all the answers
Electronegativity is defined as the relative ______ that an atom in a molecule has for shared electrons.
Electronegativity is defined as the relative ______ that an atom in a molecule has for shared electrons.
Signup and view all the answers
In a polar covalent bond, there is ______ sharing of the pair of electrons.
In a polar covalent bond, there is ______ sharing of the pair of electrons.
Signup and view all the answers
The greater the electronegativity ______, the more polar the bond.
The greater the electronegativity ______, the more polar the bond.
Signup and view all the answers
A non-polar covalent bond involves atoms that share electrons ______.
A non-polar covalent bond involves atoms that share electrons ______.
Signup and view all the answers
The bond angle for a tetrahedral shape is ______ degrees.
The bond angle for a tetrahedral shape is ______ degrees.
Signup and view all the answers
Covalent bonding and polar covalent bonding are examples of ______ bonding.
Covalent bonding and polar covalent bonding are examples of ______ bonding.
Signup and view all the answers
Intermolecular forces are the forces of attraction that exist between ______.
Intermolecular forces are the forces of attraction that exist between ______.
Signup and view all the answers
Van der Waals forces are weak attractive forces between molecules resulting from the formation of temporary ______.
Van der Waals forces are weak attractive forces between molecules resulting from the formation of temporary ______.
Signup and view all the answers
Van der Waals forces are the only forces of attraction between ______ molecules.
Van der Waals forces are the only forces of attraction between ______ molecules.
Signup and view all the answers
Dipole-Dipole forces occur between the negative pole of one polar molecule and the positive pole of another ______ molecule.
Dipole-Dipole forces occur between the negative pole of one polar molecule and the positive pole of another ______ molecule.
Signup and view all the answers
Hydrogen Bonds are particular types of dipole-dipole attractions between molecules in which Hydrogen atoms are bonded to ______, Oxygen or Fluorine.
Hydrogen Bonds are particular types of dipole-dipole attractions between molecules in which Hydrogen atoms are bonded to ______, Oxygen or Fluorine.
Signup and view all the answers
The strength of Van der Waals forces increases with the size of the ______.
The strength of Van der Waals forces increases with the size of the ______.
Signup and view all the answers
The hydrogen bond acts as a bridge between two electronegative atoms in ______ molecules.
The hydrogen bond acts as a bridge between two electronegative atoms in ______ molecules.
Signup and view all the answers
Study Notes
Chemical Bonding
- A compound is a substance made of two or more different elements combined chemically.
- Attractive forces, called chemical bonds, hold the atoms together in a compound.
- The Octet Rule describes how atoms tend to gain, lose, or share electrons to achieve an electron arrangement with eight electrons in their outermost energy level.
- Noble gases have stable electron configurations with eight or two electrons in their outermost level, so they do not react.
- Transition metals often do not follow the octet rule
- Hydrogen, lithium, and beryllium often achieve a full outer shell with just two electrons.
- An ion is a charged atom or group of atoms that has gained or lost electrons.
- Ionic bonding occurs when electrons are transferred completely from one atom to another, forming ions that attract each other.
- A cation is a positively charged ion.
- An anion is a negatively charged ion.
- An ionic bond is the force of attraction between oppositely charged ions.
Ionic Compounds: Formulas
- Chemical formulas represent compounds using element symbols and numbers to show how many atoms of each element are present.
- Ionic compounds are usually formed from metal groups I and II combining with non-metal groups VI and VII.
- Ionic compounds are neutral, so the positive and negative charges in the compound must be equal.
- Common Polyatomic ions (include their charges and formulas)
- Hydroxide (OH⁻)
- Nitrate (NO₃⁻)
- Hydrogencarbonate (HCO₃⁻)
- Permanganate (MnO₄⁻)
- Carbonate (CO₃²⁻)
- Chromate (CrO₄²⁻)
- Dichromate (Cr₂O₇²⁻)
- Sulfate (SO₄²⁻)
- Sulfite (SO₃²⁻)
- Thiosulfate (S₂O₃²⁻)
- Phosphate (PO₄³⁻)
- Ammonium (NH₄⁺)
Writing Ionic Compound Formulas
- Determine the charges of the ions involved.
- Find the lowest common multiple of the absolute values of the charges.
- Use the lowest common multiple to determine the number of each ion needed to balance the charges.
- Write the formula using the subscripts to indicate the number of each ion.
Covalent Bonding
- Covalent bonding involves the sharing of electrons between atoms.
- A molecule is a group of atoms joined together, the smallest particle of an element or compound that can exist independently.
- Single, double, or triple bonds represent the number of electron pairs shared between atoms.
- A single bond = one shared pair
- A double bond = two shared pairs
- A triple bond = three shared pairs
- Chlorine gas (Cl2) shares a pair of electrons, a single covalent bond, so Cl2 is a molecule.
- Oxygen needs two pairs of electrons (two covalent bonds) to reach a full outer shell of 8 electrons, forming a molecule (O2).
- Hydrogen gains a pair, and hydrogen atoms gain a full outer shell of 2 electrons so H2 is a molecule
Shapes of Covalent Molecules
- Use VSEPR (valence shell electron pair repulsion) theory to predict the shape of a molecule. Count the bond pairs and lone pairs around the central atom.
Electronegativity
- Electronegativity is the tendency of an atom to attract shared electrons in a covalent bond
- A large electronegativity difference indicates polar covalent bonds (unequal sharing).
- A small difference indicates nonpolar covalent bonds (equal sharing)
- Polar bonds result in a slightly positive end (δ+) and a slightly negative end (δ-)
Types of Covalent Bonds
- nonpolar covalent: bonds with equal sharing of electrons
- polar covalent: bonds with unequal sharing of electrons resulting from a difference in electronegativity between the atoms
Intermolecular Forces
- Intramolecular bonds occur within a molecule.
- Intermolecular forces occur between molecules. Examples include Van der Waals forces, dipole-dipole forces, and hydrogen bonding
- Van der Waals forces: weak attractive forces between non-polar molecules due to temporary dipoles
- Dipole-dipole forces: attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
- Hydrogen bonding: a strong type of dipole-dipole force that occurs when hydrogen is bonded to a highly electronegative atom.
- These interactions greatly affect boiling/melting point. Larger molecules generally (but not always) have higher boiling points due to stronger intermolecular forces.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Test your knowledge on the essential concepts of chemical bonding, including ionic bonds, the octet rule, and ion formation. Explore how atoms interact and bond to form compounds through various attractive forces. This quiz covers fundamental principles that are crucial for understanding chemistry.
