2.1.1, 2.1.2 Atomic Structure

• What are the three subatomic particles?

  Protons, neutrons, and electrons
• What are the position, relative mass, and relative charge of a proton?

  • Position: Nucleus
  • Relative Mass: 1
  • Relative Charge: +1
• What are the position, relative mass, and relative charge of a neutron?

  • Position: Nucleus
  • Relative Mass: 1
  • Relative Charge: 0
• What is the atomic number (Z)?

  The number of protons in the nucleus
• What are the position, relative mass, and relative charge of an electron?

  • Position: Orbitals
  • Relative Mass: 1/1800
  • Relative Charge: -1
• What is the mass number (A)?

  The total number of protons and neutrons in the atom
• How do you calculate the number of neutrons in an atom?

  Number of neutrons = A - Z
• How do isotopes compare in their chemical properties?

  Isotopes have similar chemical properties because they have the same electronic structure.
• How do isotopes differ in their physical properties?

  They may have slightly varying physical properties because they have different masses.
• What are isotopes?

  Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons.
• How is the relative atomic mass defined?

  The weighted mean mass of one atom compared to one twelfth of the mass of one atom of carbon-12.
• How is the relative isotopic mass defined?

  The mass of one isotope compared to one twelfth of the mass of one atom of carbon-12.
• How is the relative atomic mass quoted on the periodic table calculated?

  It is a weighted mean mass of all isotopes, taking into account the relative abundances of all isotopes.
• What equation is used to calculate the relative atomic mass?

  1. A.M = $\frac{\sum (\text{isotopic mass} \times \% \text{abundance})}{100}$
• What is the relative atomic mass of Mg based on the given abundance data?

  24.3
• How is the relative molecular mass defined?

  The average mass of a molecule compared to one twelfth of the mass of one atom of carbon-12.
• What are the percentage abundances of $^{63}\text{Cu}$ and $^{65}\text{Cu}$ if the relative atomic mass of copper is 63.5?


  $^{63}\text{Cu}$ = 72.5%, $^{65}\text{Cu}$ = 27.5%
• What are the percentage abundances of $^{35}\text{Cl}$ and $^{37}\text{Cl}?$


  $^{35}\text{Cl}$ = 75%, $^{37}\text{Cl}$ = 25%
• What are the percentage abundances of $^{79}\text{Br}$ and $^{81}\text{Br}?$


  $^{79}\text{Br}$ = 50%, $^{81}\text{Br}$ = 50%
• Give the ions with +1 Charge

  • Group 1 elements
  • Hydrogen
  • Silver
  • Gold
  • Ammonium $(NH_4^+)$
• Give the ions with the +2 Charge

  • Group 2 elements
  • Zinc
  • Copper (II)
  • Iron (II)
  • Tin
  • Lead
• Give the ions with charges +3

  
  

  Group 3

  Iron (III)
• Give the ion with -4 Charge

  
  

  Group 5

  Phosphate $(PO_4^{3-})$
• Give the ions with -2 Charge

  • Group 6
  • Carbonate $(CO_3^{2-})$
  • Sulfate $(SO_4^{2-})$
• Give the ions with -1 Charge

  • Group 7
  • Nitrate (NO3 -)
  • Hydroxide $(OH^-)$
• How do you determine the formula of an ionic compound from the ionic charges?

  1. Identify the ionic charges of the two ions
  2. Combine the ions together to get a neutral compound by ensuring the total positive charge cancels out the total negative charge
• What are the key features of ionic equations?

  They show only the ions that are reacting and omit spectator ions.
• What are spectator ions?

  Ions that are not changing state or oxidation number during a reaction.