AP CHEM Trimester 1 Review

• What does Coulomb's law describe?


  The electrical force between two charged objects
• What is the formula for Coulomb's law?


  F = ke * (q1 q2/R^2)
• What is the approximate value of the constant \( K \) in Coulomb's law?


  Approximately \( 9 * 10^9) N m²/C²
• What types of electrical charges can matter have?


  Positive, negative, or neutral
• What happens when two like charges are brought close together?


  They repel each other
• How do neutral charges interact with electrically charged objects?


  Neutral charges do not interact with charged objects
• How does the distance between two charges affect the force between them?


  The closer the charges, the stronger the force
• What does it mean when the force between two charges is positive?


  It indicates a repulsive force
• What happens when one charge is neutral in Coulomb's law?


  The force between the charges is zero
• What is the effect of doubling the distance between two charges on the force?


  The force becomes one quarter of the original force
• What is the significance of the \( r^2 \) term in Coulomb's law?


  It indicates that the force is inversely proportional to the square of the distance
• How can the constant \( K \) be expressed in terms of \( \epsilon_0 \)?


  K = \frac{1}{4 \pi \epsilon_0}
• What is the approximate value of the vacuum permittivity \( \epsilon_0 \)?


  Approximately \( 8.85 \times 10^{-12} \) C²/(N m²)
• What are the key principles of Coulomb's law?


  • The force between two charges is proportional to the product of their charges.
  • Like charges repel, while opposite charges attract.
  • The force is inversely proportional to the square of the distance between the charges.
• What happens to the force if the distance between two charges is halved?

  • The force quadruples.
  • This is due to the inverse square relationship in Coulomb's law.
• What is the periodic table of elements?


  It is an arrangement of elements that reveals patterns about how nature operates.
• What did Mendeleev predict about the gaps in his periodic table?


  He predicted that there must be undiscovered elements that would fit into those gaps.
• Why do elements in the same group behave similarly?


  They have the same number of valence electrons.
• How many valence electrons do elements in group one have?


  One valence electron
• What happens to atomic size as you move down the periodic table?


  Atomic size increases because additional shells are added.
• What trend occurs in atomic radius as you move to the right across a period?


  Atomic radius decreases due to increased nuclear charge.
• How does ionic radius differ from atomic radius?


  Ionic radius can increase with the addition of electrons and decrease with the removal of electrons.
• What is ionization energy?


  It is the energy required to remove an electron from an atom.
• How does the distance of an electron from the nucleus affect ionization energy?


  The farther away an electron is from the nucleus, the easier it is to remove it, resulting in lower ionization energy.
• Which element has a very low ionization energy due to its large atomic size?


  Francium
• Why does helium have a high ionization energy?


  Helium has a full outer shell and its electrons are very close to the nucleus, making it stable and requiring more energy to ionize.
• What happens to successive ionization energies as more electrons are removed?


  Successive ionization energies increase because the atom becomes less stable with each electron removed.
• What significant change occurs in ionization energy after removing the last electron in a shell?


  There is a huge jump in ionization energy because the atom reaches a noble gas electron configuration.
• What is the reason for the dip in ionization energy from nitrogen to oxygen?


  The dip occurs due to orbital symmetry, where nitrogen's half-full 2p orbitals provide special stability.
• What does electron affinity measure?


  Electron affinity measures how much an atom wants to gain an electron.
• Which element has the highest electron affinity?


  Fluorine
• Why do noble gases have low electron affinity?


  Noble gases have full shells and do not want to gain electrons.
• What is electronegativity?


  Electronegativity is the ability of an atom to hold electrons tightly.
• How does electronegativity change across the periodic table?


  Electronegativity increases as you move to the right across the periodic table.
• What are the periodic trends to remember in the periodic table?


  • Atomic radius increases down the table and decreases to the right.
  • Ionization energy increases to the right.
  • Electron affinity increases to the right.
  • Electronegativity increases to the right.
• What are the three main types of bonding in elements and compounds?

  Covalent bonding, ionic bonding, and metallic bonding
• How does covalent bonding occur?


  Atoms share electrons so their outer shells overlap
• In which types of elements does covalent bonding occur?


  Only in non-metals
• What are the two types of covalent bonding?


  Simple covalent and giant covalent
• What is an example of a simple covalent molecule?


  CH₄, H₂O, or CO₂