Based on the information requested in the worksheet, here is the completed data for each of the nine elements listed. The values are based on standard scientific data for the most common isotopes of these elements.
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Hydrogen (H)
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Atomic Number: 1
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Atomic Mass: 1.008
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Symbol: H
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# of protons: 1
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# of neutrons: 0 (for the most common isotope, Hydrogen-1)
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# of electrons: 1
Boron (B)
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Atomic Number: 5
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Atomic Mass: 10.81
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Symbol: B
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# of protons: 5
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# of neutrons: 6 (for the most common isotope, Boron-11)
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# of electrons: 5
Aluminum (Al)
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Atomic Number: 13
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Atomic Mass: 26.98
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Symbol: Al
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# of protons: 13
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# of neutrons: 14 (for the only stable isotope, Aluminum-27)
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# of electrons: 13
Sulfur (S)
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Atomic Number: 16
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Atomic Mass: 32.06
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Symbol: S
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# of protons: 16
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# of neutrons: 16 (for the most common isotope, Sulfur-32)
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# of electrons: 16
Oxygen (O)
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Atomic Number: 8
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Atomic Mass: 16.00
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Symbol: O
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# of protons: 8
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# of neutrons: 8 (for the most common isotope, Oxygen-16)
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# of electrons: 8
Helium (He)
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Atomic Number: 2
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Atomic Mass: 4.003
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Symbol: He
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# of protons: 2
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# of neutrons: 2 (for the most common isotope, Helium-4)
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# of electrons: 2
Potassium (K)
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Atomic Number: 19
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Atomic Mass: 39.10
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Symbol: K
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# of protons: 19
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# of neutrons: 20 (for the most common isotope, Potassium-39)
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# of electrons: 19
Sodium (Na)
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Atomic Number: 11
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Atomic Mass: 22.99
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Symbol: Na
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# of protons: 11
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# of neutrons: 12 (for the only stable isotope, Sodium-23)
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# of electrons: 11
Carbon (C)
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Atomic Number: 6
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Atomic Mass: 12.01
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Symbol: C
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# of protons: 6
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# of neutrons: 6 (for the most common isotope, Carbon-12)
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# of electrons: 6
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Explanation:
The worksheet asks for fundamental properties of atoms.
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Atomic Number: This is the number of protons in the nucleus of an atom and defines the element. It is always a whole number.
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Atomic Mass: This is the average mass of all the naturally occurring isotopes of an element, weighted by their abundance. It is usually not a whole number.
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Symbol: This is the one- or two-letter abbreviation for the element's name.
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Number of Protons: This is equal to the atomic number.
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Number of Electrons: In a neutral atom (which is assumed unless otherwise specified), the number of electrons equals the number of protons.
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Number of Neutrons: This is calculated by rounding the atomic mass to the nearest whole number (the mass number of the most common isotope) and subtracting the atomic number (number of protons). For example, for Oxygen: Mass Number ≈ 16, Atomic Number = 8, so Neutrons = 16 - 8 = 8.
Parent Tip: Review the logic above to help your child master the concept of periodic table fun worksheet.
