The table below shows the number of protons, neutrons, electrons and the mass numbers of some atoms Q, R, Y and Z. The letters used are not the usual symbols of the elements.

Physics
The table below shows the number of protons, neutrons, electrons and the mass numbers of some atoms Q, R, Y and Z. The letters used are not the usual symbols of the elements.

ScanSolve AI Answer

1.i. Complete the table above.

Step 1: Determine the number of electrons for Q, R, Y, and Z. For a neutral atom, the number of electrons is equal to the number of protons.

  • Q: Protons = 6, so Electrons = 6.
  • R: Protons = 6, so Electrons = 6.
  • Y: Electrons = 5, so Protons = 5.
  • Z: Electrons = 6, so Protons = 6.

Step 2: Determine the mass number for Q, R, Y, and Z. Mass number = Protons + Neutrons.

  • Q: Protons = 6, Neutrons = 6, so Mass = 6+6=126 + 6 = 12.
  • R: Protons = 6, Neutrons = 8, so Mass = 6+8=146 + 8 = 14.
  • Y: Protons = 5, Mass = 14, so Neutrons = 14−5=914 - 5 = 9.
  • Z: Protons = 6, Neutrons = 6, so Mass = 6+6=126 + 6 = 12.

The completed table is: | Atom | Protons | Neutrons | Electrons | Mass | | :--- | :------ | :------- | :-------- | :--- | | Q | 6 | 6 | 6 | 12 | | R | 6 | 8 | 6 | 14 | | Y | 5 | 9 | 5 | 14 | | Z | 6 | 6 | 6 | 12 |

1.ii. Identify a pair of isotopes from the atoms represented by letters Q, R, Y and Z. Isotopes are atoms of the same element, meaning they have the same number of protons but different numbers of neutrons.

  • Q has 6 protons and 6 neutrons.
  • R has 6 protons and 8 neutrons.
  • Y has 5 protons and 9 neutrons.
  • Z has 6 protons and 6 neutrons. Atoms Q and R both have 6 protons but different numbers of neutrons (6 for Q, 8 for R). Therefore, Q and R are isotopes.

The pair of isotopes is QandR\boxed{Q and R}.

1.ii. If the two isotopes occur in nature in equal proportions, calculate the relative atomic mass. The two isotopes are Q (mass number 12) and R (mass number 14). "Equal proportions" means each isotope has an abundance of 50%. Relative atomic mass = (MassofQ×AbundanceofQ)+(MassofR×AbundanceofR)(Mass of Q \times Abundance of Q) + (Mass of R \times Abundance of R) Relativeatomicmass=(12×0.50)+(14×0.50)Relative atomic mass = (12 \times 0.50) + (14 \times 0.50) Relativeatomicmass=6+7Relative atomic mass = 6 + 7 Relativeatomicmass=13Relative atomic mass = 13 The relative atomic mass is 13\boxed{13}.

1.iii. Z reacts with oxygen to form a compound. Write an equation for the reaction. Atom Z has 6 protons, which means it is Carbon (C). Carbon reacts with oxygen (O2\text{O}_2) to form carbon dioxide (CO2\text{CO}_2) under complete combustion. C(s)+O2(g)→CO2(g)C_{(s)} + O_{2(g)} \to CO_{2(g)} The equation for the reaction is C(s)+O2(g)→CO2(g)\boxed{C_{(s)} + O_{2(g)} \to CO_{2(g)}}.

1.iv. Draw a dot and cross diagram for the bonding in the compound formed between Z and oxygen. Atom Z is Carbon (C), with 4 valence electrons. Oxygen (O) has 6 valence electrons. In carbon dioxide (CO2\text{CO}_2), carbon forms two double covalent bonds with two oxygen atoms.

O××⋅⋅C⋅⋅××O\begin{array}{c} O \\ \times \times \\ \cdot \cdot C \cdot \cdot \\ \times \times \\ O \end{array}

The dot and cross diagram for CO2\text{CO}_2 is:

\begin{array}{c} \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \
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