atomic structure worksheet\nlist the 3 subatomic particles, their charges, masses and where in the atom they…

atomic structure worksheet\nlist the 3 subatomic particles, their charges, masses and where in the atom they are located in the chart below.\ndescribe how to determine the number of each subatomic particle in an atom below.\nproton:\nelectron:\nneutron:\nfill in the chart for the elements below. round all atomic masses to the nearest whole number.\nelement symbol (z) atomic number (a) atomic mass # of protons # of electrons # of neutrons\nsodium na 11 22.990 11 11 12\ncopper cu 29 63.546 29 29\nchlorine cl 17 35. 17\nsilver ag 47 107.868\npb 82 207.2\ncalcium ca 20 40.078\nhafnium hf 72 178.49\nradon\n 93 52\nuranium\npotassium

atomic structure worksheet\nlist the 3 subatomic particles, their charges, masses and where in the atom they are located in the chart below.\ndescribe how to determine the number of each subatomic particle in an atom below.\nproton:\nelectron:\nneutron:\nfill in the chart for the elements below. round all atomic masses to the nearest whole number.\nelement symbol (z) atomic number (a) atomic mass # of protons # of electrons # of neutrons\nsodium na 11 22.990 11 11 12\ncopper cu 29 63.546 29 29\nchlorine cl 17 35. 17\nsilver ag 47 107.868\npb 82 207.2\ncalcium ca 20 40.078\nhafnium hf 72 178.49\nradon\n 93 52\nuranium\npotassium

Answer

Explanation:

Step1: Identify sub - atomic particle properties

Proton: charge = + 1, mass ≈ 1 amu, located in nucleus. Electron: charge=-1, mass ≈ 0 amu, located in electron - cloud around nucleus. Neutron: charge = 0, mass ≈ 1 amu, located in nucleus.

Step2: Determine number of sub - atomic particles

  • Proton: The number of protons is equal to the atomic number (Z) of the element.
  • Electron: In a neutral atom, the number of electrons is equal to the number of protons.
  • Neutron: Number of neutrons = Atomic mass (A) (rounded to nearest whole number)-Atomic number (Z).

Step3: Fill in the chart for elements

  • Sodium (Na): Z = 11, A≈23. Protons = 11, Electrons = 11, Neutrons=23 - 11 = 12.
  • Copper (Cu): Z = 29, A≈64. Protons = 29, Electrons = 29, Neutrons=64 - 29 = 35.
  • Chlorine (Cl): Z = 17, A≈35. Protons = 17, Electrons = 17, Neutrons=35 - 17 = 18.
  • Silver (Ag): Z = 47, A≈108. Protons = 47, Electrons = 47, Neutrons=108 - 47 = 61.
  • Lead (Pb): Z = 82, A≈207. Protons = 82, Electrons = 82, Neutrons=207 - 82 = 125.
  • Calcium (Ca): Z = 20, A≈40. Protons = 20, Electrons = 20, Neutrons=40 - 20 = 20.
  • Hafnium (Hf): Z = 72, A≈179. Protons = 72, Electrons = 72, Neutrons=179 - 72 = 107.
  • Radon (Rn): Assume some values. If we consider a common isotope, for example, if Z = 86 and we need more information about the specific isotope for accurate A value. But if we assume a typical A value around 222, Protons = 86, Electrons = 86, Neutrons=222 - 86 = 136.
  • Uranium (U): Z = 92, for example, for U - 238 isotope, A = 238. Protons = 92, Electrons = 92, Neutrons=238 - 92 = 146.
  • Potassium (K): Z = 19, A≈39. Protons = 19, Electrons = 19, Neutrons=39 - 19 = 20.

Answer:

Element Symbol Atomic Number (Z) Atomic Mass (A) (rounded) # of Protons # of Electrons # of Neutrons
Sodium Na 11 23 11 11 12
Copper Cu 29 64 29 29 35
Chlorine Cl 17 35 17 17 18
Silver Ag 47 108 47 47 61
Lead Pb 82 207 82 82 125
Calcium Ca 20 40 20 20 20
Hafnium Hf 72 179 72 72 107
Radon Rn 86 222 (assumed) 86 86 136
Uranium U 92 238 (assumed for U - 238) 92 92 146
Potassium K 19 39 19 19 20