Answer to Each Step Answer after Arithmetic 1. Begin with number of cm equal to
ID: 699330 • Letter: A
Question
Answer to Each Step
Answer after Arithmetic
1. Begin with number of cm equal to one inch (to two decimal places).
2.54 cm
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2. Multiply by the number of mL in 0.10 L.
1 L = 1000 ml; therefore, 0.10 L = (0.10 L)*(1000 mL/1 L) = 100 mL
2.54*100 = 254
3. Add the number of neutrons in a carbon-14 atom.
Carbon has atomic number 6; hence there are 6 protons in carbon. The number of neutrons in carbon-14 is given by (mass number) – (number of protons) = 14 – 6 = 8.
254 + 8 = 262
4. Subtract the number of electrons in a filled f sublevel.
There are 7 f subshells and each subshell can accommodate two electrons; hence, the total number of electrons in f subshells = 2*7 = 14
262 – 14 = 248
5. Divide by the total number of protons and neutrons in an alpha particle.
An alpha particle is dipositively charge helium nucleus, i.e, 4He2. The number of protons and neutrons equals the mass number of He which is 4.
248/4 = 62
6. Multiply by the number of 4d electrons in a zirconium atom.
Zirconium has two 4d electrons.
62*2 = 124
7. Divide by the number of atoms in a bromine molecule.
A bromine molecule has 2 atoms.
124/2 = 62
8. Subtract the number of protons in the nucleus of tin atom.
Tin has atomic number 50; hence, there are 50 protons in the nucleus of tin.
62 – 50 = 12
9. Divide by the numerical value of the charge on a phosphide ion.
A phosphide ion has charge -3; we will consider the numerical value, i.e, 3.
12/3 = 4
10. Multiply by the IUPAC group number of the alkaline earth metals.
The alkaline earth metals occur in Group II of the periodic table. Consider the numerical value, i.e, 2.
4*2 = 8
11. Multiply by the numerical value of the charge on an aluminum ion.
An aluminum ion has charge +3. Multiply by 3.
8*3 = 24
12. Subtract the atomic mass of fluorine.
The atomic mass of fluorine is considered to be 19.
24 – 19 = 5
Final Answer
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5
Answer to Each Step
Answer after Arithmetic
1. Begin with number of cm equal to one inch (to two decimal places).
2.54 cm
-
2. Multiply by the number of mL in 0.10 L.
1 L = 1000 ml; therefore, 0.10 L = (0.10 L)*(1000 mL/1 L) = 100 mL
2.54*100 = 254
3. Add the number of neutrons in a carbon-14 atom.
Carbon has atomic number 6; hence there are 6 protons in carbon. The number of neutrons in carbon-14 is given by (mass number) – (number of protons) = 14 – 6 = 8.
254 + 8 = 262
4. Subtract the number of electrons in a filled f sublevel.
There are 7 f subshells and each subshell can accommodate two electrons; hence, the total number of electrons in f subshells = 2*7 = 14
262 – 14 = 248
5. Divide by the total number of protons and neutrons in an alpha particle.
An alpha particle is dipositively charge helium nucleus, i.e, 4He2. The number of protons and neutrons equals the mass number of He which is 4.
248/4 = 62
6. Multiply by the number of 4d electrons in a zirconium atom.
Zirconium has two 4d electrons.
62*2 = 124
7. Divide by the number of atoms in a bromine molecule.
A bromine molecule has 2 atoms.
124/2 = 62
8. Subtract the number of protons in the nucleus of tin atom.
Tin has atomic number 50; hence, there are 50 protons in the nucleus of tin.
62 – 50 = 12
9. Divide by the numerical value of the charge on a phosphide ion.
A phosphide ion has charge -3; we will consider the numerical value, i.e, 3.
12/3 = 4
10. Multiply by the IUPAC group number of the alkaline earth metals.
The alkaline earth metals occur in Group II of the periodic table. Consider the numerical value, i.e, 2.
4*2 = 8
11. Multiply by the numerical value of the charge on an aluminum ion.
An aluminum ion has charge +3. Multiply by 3.
8*3 = 24
12. Subtract the atomic mass of fluorine.
The atomic mass of fluorine is considered to be 19.
24 – 19 = 5
Final Answer
-
5
Explanation / Answer
Please answer all quetions
hemical Arithmetic eriodic Table 3 und each answer to the nearest whole number less indicated otherwise. Name (Ony She h Answer to Each Step Answer after Arithmetic 1. Begin with the number of em equal to one inch (to two decimal places). 2. Multiply by the number of mL in 0.10 L 3. Add the number of neutrons in a carbon-14 atom. 4. Subtract the number of electrons in a filled f sublevel. 5. Divide by the total number of protons and neutrons in an alpha particle. Multiply by the number of 4d electrons in a zirconium atom 7. Divide by the number of atoms in a bromine molecule. 8. Subtract the number of protons in the nucleus of a tin atom. 9. Divide by the numerical value of the charge of a phosphide ion. 10. Multiply by the IUPAC group number of the alkaline earth metals. 11. Multiply by the numerical value of the charge on an aluminum ion. 2. Subtract the atomic mass of fluorine. al AnswerRelated Questions
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