AP Chemistry Electronegativity Quiz

Questions and Answers

What is electronegativity?

Ability of an atom in a molecule to attract shared electrons to itself (correct)

Ability of an atom to lose electrons

Measure of an atom's size

None of the above

What is the trend in electronegativity from left to right on the periodic table?

Increases

What is the trend in electronegativity down a group on the periodic table?

Decreases

What is a chemical bond?

Attraction between the nucleus of one atom and the electron of another Signup and view all the answers

What type of bond involves transferring electrons between a metal and a nonmetal?

Ionic bond Signup and view all the answers

What type of bond involves sharing electrons between two nonmetals?

Covalent bond Signup and view all the answers

What does it mean if electrons are shared equally?

Nonpolar Signup and view all the answers

What does it mean if electrons are shared unequally?

Polar Signup and view all the answers

What is a metallic bond?

Electrons not associated with a single atom or molecule (delocalized electrons) Signup and view all the answers

How does a covalent bond work between nonmetals?

Nucleus is positive, electrons are attached to each individual atom Signup and view all the answers

How does a metallic bond work between metals?

Metals are cations, mobile electrons in a sea can move around metals Signup and view all the answers

What causes metallic bonding?

Attraction between protons and electrons Signup and view all the answers

What is bond polarity?

Difference in electronegativity values of two elements Signup and view all the answers

What is the charge of an element with high electronegativity?

Partially negative Signup and view all the answers

What is the charge of an element with low electronegativity?

Partially positive Signup and view all the answers

What does a dipole arrow indicate?

Points towards more electronegative atom Signup and view all the answers

What is a chemical bond a balance between?

Attraction and repulsion Signup and view all the answers

What is intermolecular distance?

Distance between nuclei of atoms measured in pm, x-axis of a potential energy curve Signup and view all the answers

What does the y-axis of a potential energy curve measure?

Potential energy measured in kJ/mol Signup and view all the answers

What is the position of atoms where potential energy is 0?

Atoms far apart Signup and view all the answers

What is the position of atoms where potential energy is decreasing?

Atoms are closer together Signup and view all the answers

What is the position of atoms with the lowest potential energy?

Atoms are together Signup and view all the answers

What is the position of atoms where potential energy is increasing?

Atoms overlap Signup and view all the answers

What is bond energy?

Energy required to break the bond between atoms Signup and view all the answers

What does an endothermic process indicate about bond energy?

Causes bond energy to be a positive value that requires energy Signup and view all the answers

What does bond length represent?

Intermolecular difference of a potential energy curve, x-axis Signup and view all the answers

What does bond energy represent in a potential energy curve?

Potential energy of a potential energy curve, y-axis Signup and view all the answers

What is an ionic bond?

Electrostatic attraction between a cation and anion Signup and view all the answers

What does Coulomb's law explain?

Interactions between cations and anions Signup and view all the answers

What causes a larger force of attraction?

Larger ion force causes this Signup and view all the answers

What causes a smaller force of attraction?

Greater distance between charges causes this Signup and view all the answers

Order the following bonds in terms of strength from weakest to strongest:

Single = weakest Double = intermediate Triple = strongest Signup and view all the answers

Order the following bonds in terms of length from shortest to longest:

Triple = shortest Double = intermediate Single = longest Signup and view all the answers

How do ionic solids conduct electricity?

Charged particles are free to move Signup and view all the answers

What state of matter cannot conduct electricity?

Solid Signup and view all the answers

What state of matter can conduct electricity?

Molten (melted) Signup and view all the answers

What characterizes a metallic bond?

Positive metal ions surrounded by a 'sea of mobile electrons' (delocalized electrons) Signup and view all the answers

What are properties of a metallic bond?

Good conductor of electricity, malleable (bendable), ductile (pulled in a wire) Signup and view all the answers

What is the difference between ionic and metallic bonds in conducting electricity?

Ionic bonds conduct electricity through cations and anions being free to move, metallic bonds conduct electricity through valence electrons being free to move Signup and view all the answers

Study Notes

Electronegativity and Trends

Electronegativity measures an atom's ability to attract shared electrons in a molecule.
Increases from left to right on the periodic table, indicating greater nuclear charge.
Decreases down a group due to increased distance between the nucleus and valence electrons.

Chemical Bonds

A chemical bond is formed by the attraction between the nucleus of one atom and the electrons of another.
Ionic bonds involve transferring electrons, typically between metals and nonmetals.
Covalent bonds involve sharing electrons, which predominantly occurs between nonmetals.

Bond Types and Characteristics

Nonpolar bonds occur when electrons are shared equally between atoms.
Polar bonds occur when electrons are shared unequally, leading to partial charges.
Metallic bonds feature delocalized electrons that are not associated with a single atom, allowing mobility.

Bond Polarity and Charge

Bond polarity relates to the difference in electronegativity between two bonded atoms.
Atoms with high electronegativity acquire a partially negative charge, while those with low electronegativity have a partially positive charge.
A dipole arrow indicates the direction of increased electronegativity, pointing toward the more electronegative atom.

Energy Considerations in Bonds

A chemical bond is characterized by a balance between attraction and repulsion forces.
Potential energy is measured on the y-axis of a potential energy curve, while atomic separation distance is on the x-axis.
Atoms far apart display zero potential energy, while closer atoms experience decreasing potential energy due to attraction.

Stability and Bond Length

Atoms in a stable configuration are at the lowest potential energy with balanced attractions and repulsions.
Atoms that overlap strongly experience high repulsion, leading to increased potential energy and instability.
Bond length is represented on the potential energy curve’s x-axis, indicating the distance at which atoms can bind effectively.

Bond Energy and Types

Bond energy is the amount of energy needed to break a bond between atoms.
Endothermic processes involve energy input, resulting in positive bond energy values.
Ionic bonds result from the electrostatic attraction between cations and anions.

Coulomb's Law in Ionic Interactions

Coulomb's law describes the interactions between charged particles, with larger ions creating a stronger force of attraction.
Greater separation distance between charges leads to diminished attractive forces.

Strength and Length of Bonds

Bonds are ranked from weakest to strongest as single, double, and triple bonds.
Conversely, bonds are ranked from shortest to longest as triple, double, and single bonds.

Electrical Conductivity in Ionic and Metallic Compounds

Ionic solids conduct electricity when molten, as charged particles (cations and anions) are free to move.
In solid form, ionic compounds do not conduct electricity due to fixed positions of ions.
Metallic bonds allow conduction of electricity due to the presence of mobile valence electrons.

Properties of Metallic Bonds

Metallic bonds create substances that are good conductors of electricity, malleable, and ductile.
The structure consists of positive metal ions within a sea of delocalized electrons, contributing to their unique properties.

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Description

Test your knowledge on electronegativity with this quiz focusing on key terms from AP Chemistry. Learn about trends in electronegativity across the periodic table and the concept of chemical bonds. Perfect for AP Chemistry students preparing for exams!