Download Atomic structure practice worksheet Atomic Calculating the atomic

Atomic structure practice worksheet
Calculating the atomic mass from the Relative Abundance of Isotopes.
1. Boron has two naturally occurring isotopes with masses of 10.0129 amu which occupies 19.91
percent and another isotope of 11.0093 amu and occupying 80.09 percent. Calculate the
average atomic mass of Boron (The number listed on the periodic table)
2. Bromine has two isotopes with the first having a mass of 78.918336 amu and occupying 50.69%
and the second isotope having a mass of 80.916289 amu and occupying 49.31%. What is the
average atomic mass of bromine?
3. Verify the atomic mass of Chlorine as 35.45 amu knowing that chlorine has two isotopes of the
following data:
35
Cl = 34.96885 amu and percent abundance of 75.77%
37
Cl = 36.96590 amu and percent abundance of 24.23%
4. Verify the atomic mass of Magnesium as 24.31 amu knowing the following information:
24
Mg = 23.985042 amu and percent abundance of 78.99%
25
Mg = 24.985837 amu and percent abundance of 10.00%
26
Mg = 25.982593 amu and percent abundance of 11.01%
Atomic Spectra
5. How is an atomic emission spectrum of an element produced? What does each line in the
emission spectrum indicate?
6. Compare the energy of an electron in the ground state and an electron in the excited state.
7. When an electron falls from a higher energy level to a lower energy level, how is the energy
released?
8. List the seven colors of the visible light spectrum in order of increasing energy.
9. What is a photon? What is the difference between a photon of yellow light and a photon of
violet light?
10. Describe the Bohr model of the hydrogen atom.
11. How are frequency and wavelength of an electromagnetic wave related?
Atomic
12. If each orbital can hold a maximum of two electrons, how many electrons can each of the
following hold? a. 2s b. 5p c. 4f d. 3d e. 4d
13. What is the shape of an s orbital?
14. How many s orbitals can there be in an energy level?
15. How many electrons can occupy an s orbital?
16. What is the shape of a p orbital?
17. How many p orbitals can there be in an energy level?
18. Which is the lowest energy level that can have an s orbital?
19. Which is the lowest energy level that can have a p orbital?
20. Is it possible for two electrons in the same atom to have exactly the same set of quantum
numbers?
21. Distinguish between an atom in its ground state and an excited atom.
22. How many d orbitals can there be in an energy level?
23. How many d electrons can there be in an energy level?
24. Which is the lowest energy level having d orbitals?
25. How many energy levels are partially or fully occupied in a neutral atom of calcium?
26. Why do the fourth and fifth series of elements contain 18 elements, rather than 8 as do the
second and third series?
27. Which sublevels of the 3rd energy level are filled (a) in the element argon (b) in the element
krypton?
28. Why does it take more energy to remove an electron from Al+ than from Al?
29. What does the term principal quantum number refer to?
30. What is meant by the electron configuration of an atom?
31. What is the maximum number of electrons that can be present in an atom having three principal
energy levels?
1st Ionization NRG
2500
2000
1500
1000
500
0
Li
Be
B
C
N
O
F
Ne
32. Explain how the table above is evidence for the existence of different orbitals in an atom.