CHEMIS

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1.

Subatomic Particle Mass Charge Location

Proton 1 + Nucleus

Neutron 1 No Charge Nucleus

Electron 0 - Outside Nucleus

2. The atomic number of an element is defined by its number of ( protons / neutrons / electrons ).

 

3. What is the name for atoms of an element that have different masses or number of neutrons? ISOTOPE

4. What isotope has 8 protons and 10 neutrons? Oxygen-18

5. IDENTIFY THE FOLLOWING FOR:

atomic number 20 mass number 41

 protons 20 electrons (20-2) 18 neutrons (41-20) 21

6. In a neutral atom, what subatomic particles are the SAME?

Protons = Electrons

 

7. What is the smallest particle of an element that maintains the properties of the element?

Atom

8. A neutral atom of an element contains 12 electrons. What is the identity of this element?

Mg

9. What is the name of the element that has an atomic number of 4?

Beryllium

10. What do the dots represent in a Lewis Dot Diagram?

Valence Electrons

11. Average atomic mass is the ( actual / weighted ) average of all the isotopes of an element.

12. IDENTIFY IF ATOM #1 AND #2 ARE THE SAME ELEMENT OR DIFFERENT ELEMENTS USING THE INFORMATION IN THE TABLE.

  Atom #1 Atom #2 Same or Different

A.  3 protons, 3 neutrons

3 protons,4 neutrons Same

B.   3 protons, 3 neutrons

4 protons, 4 neutrons Different

C.   4 protons, 4 neutrons

3 protons, 4 neutrons Different

D.   3 protons, 4 neutrons

4 protons, 3 neutrons Different

13. Which isotope of Carbon is the most abundant, naturally occurring one?

a. Carbon-14 b. Carbon-13 C. Carbon-12

  

14. What is the atomic mass of silicon if 92.21% of its atoms have a mass of 27.977u, 4.70% have mass 28.976u, and 3.09% have mass 29.974u?

.9221 x 27.977 = 25.80

.0470 x 28.976 = 1.36 +

.0309 x 29.974 = 0.93

28.1 amu

15. FIND THE AVERAGE ATOMIC MASS OF KRYPTON USING THE DATA TABLE BELOW:Isotopic

massAbundance

(Percentage) ÷ 100

Mass x Percentage

Answer77.920u x 0.350% = .00350 = 0.27

79.916u x 2.27% = .0227 = 1.81

81.913u x 11.56% = .1156 = 9.47

82.914u x 11.55% = .1155 = 9.58

83.912u x 56.90% = .5690 = 47.75

85.911u x 17.37% = .1737 = 14.92Answer: 83.80 amu

16. FILL IN THE DATA TABLE BELOW WITH THE MISSING INFORMATION:

Sublevel Number Orbitals Total Number of Electrons in

Sublevel if ALL Orbitals are FULL

s 1 2

p 3 6

d 5 10

f 7 14

17. Identify the # of protons 1 , neutrons 2 and electrons 1 for

18. Write the full electron configurations for:

Potassium (K) 1s2 2s2 2p6 3s2 3p64s1 Sodium (Na) 1s2 2s2 2p6 3s1

Neon (Ne) 1s2 2s2 2p6 Boron (B) 1s2 2s2 2p1

 

19. List all of the elements that will have a ground-state electron configuration that ends in s1?

H, Li, Na, K, Rb, Cs, Fr 

20. List all of the elements that will have a ground-state electron configuration that ends in p1?

B, Al, Ga, In, Tl

21. IDENTIFY THE FOLLOWING ELEMENTS:

1s2 Helium 1s2 2s2 2p6 3s2 3p3 Phosphorous

 

[Ne] 3s2 3p6 Argon [Ne] 3s2 3p4 Sulfur

 

[Ar] 4s2 3d10 4p2 Germanium [Ar] 4s2 3d10

4p5 Bromine

22. Which element, in its ground state, has the following Orbital Diagram Below? Carbon

 

 

23. Electrons in an orbital must have ( opposite / same / no ) spin.

 

24. Which group of elements on the periodic table can we use for abbreviated electron configurations?

Noble Gases

 

25. The electrons in the outer shell (highest energy level) are called: Valence Electrons

26. How many valence electrons does each of the following have?

 

Ga - 3 Li- 1 As - 5 Xe - 8

 

Mg - 2 O- 6 C - 4 F - 7

 

27. An atom that has different number

of electrons and protons is an

( isotope / atom / ion ).

29. Identify the following for magnesium-27

  Protons: 12 Neutrons: (27-12) 15 Electrons: 12

  Mass Number: 27 Atomic Number: 12

 

30. Identify the number of electrons in the following:

Cu+1 (29-1) = 28 P-3 (15+3) = 18

F-1 (9+1) = 10 Co+3 (27-3) = 24

Fe+2 (26-2) = 24 Zn+2 (30-2) = 28