Download Name: Date: ______ Period: _____ Chemistry 1st semester final

Name: ____________________________
Date: ___________ Period: _____
Chemistry 1st semester final exam review Part 2
KEY
Unit 3 & 4 Chapter 4, 5, 6 Atomic Structure, Theory and Periodic Trends
Atomic Theory
1. Whose model was nicked name the plum pudding model?JJ Thompson
2. What atomic model(s) could account for internal structure, empty space, and matter giving off energy but
not the stability of the atom?Rutherford and Nagoka
3. For each person listed below draw and label their atomic model. tell what the model could and could
not account for.
Illustration
Could
Could Not
Name
Dalton
Billiard ball model
Different masses
Elements were tiny
particles
Internal structure
Thought atom was
smallest particle
Internal structure
Light given off
Different masses
Empty space
formation of ions
Empty space
Internal structure
Formation of ions
Light given off
Different masses
Empty space
Internal structure
Formation of ions
Light given off
Different masses
Energy levels of e-
Not stable
Solid Spear
Thomson
Plum pudding
Positive Jelly
With negative
“plums”
Rutherford
Jimmy neutron
Bohr
1st level = 2 e2nd level = 8 e3rd level = 18 e-
Only worked for
hydrogen
Subatomic Particle Review
1. What subatomic particle determines the identity of an element? Proton
2. What subatomic particle determines the chemical properties of an atom? Electron (valance Electrons)
3. What subatomic particles have an electrical charge?
Protons and electrons
4. What do we call atoms that have gained or lost electrons?
ions
5. What do we call atoms of the same element that have different atomic masses? isotopes
6. What do we call atoms of the same element that have different numbers of neutrons?
isotopes
7. An element has an atomic number of 80. How many protons and electrons are in an atom of the element?
Atomic # 80 = Mercury, has 80 p+, 80e-, and 121 n (based on mass on table)
8. How many protons, neutron, and electrons does U-234 have?is isotope, 92 p+, 92e-, 142 n
9. How many protons, neutron, and electrons does I-128 have?is isotope 53p+, 53 e-, 105 n
10. How many protons, neutron, and electrons does Ca+2 have?is ion 20p+, 18 e-, 20 n (based on mass on
table)
11. How many protons, neutron, and electrons does N-3 have?is ion 7p+, 10 e-, 7 n (based on mass on table)
12. How many protons, neutron, and electrons does Pb-210 have?is isotope, 82 p+, 82 e-, 128 n
13. What element has 21 protons and 24 neutrons? Element # 21 is Scandium and will have mass of 45 amu
14. What cation has 10 electrons?Cations have lost electons so it is either Na+1, Mg+2, or Al+3
15.
What anion has 10 electrons?Anions have gained electrons so it is either C-4, N-3, O-2, or F-1
16. Subatomic Particle summary
Subatomic
particle
Proton
Electron
Neutron
Symbol
p
en
Charge
+1
-1
No charge
Mass
1 amu
Discovered by
Year
Experiment
Rutherford
1911
Thompson
1887
Chadwick
1932
Gold Foil Experiment
Response of cathode ray to
magnetic and electric fields
Bombarded Be w/beta
radiation and a neutron was
released
amu
1 amu
Electron Configuration
17. How many different orbitals does the following sub-levels have:
a. S sub level
1 orbital
b. P sub level
3 orbitals
c. D sub level
5 orbitals
d. F sub level
7 orbitals
18. How many electrons can each sub-level hold(each orbital can hold AT MOST 2 electrons)
a. S sub level
2 electrons
b. P sub level
6 electrons
c. D sub level
10 electrons
d. F sub level
14 electrons
19. How many paired and unpaired P electrons does Fluorine have?
↓↑ ↓↑ ↓↑ ↓↑ ↓
Has: 2 pairs and 1 unpaired P electron
1𝑠 2𝑠
2𝑝
20. How many paired and unpaired electrons does Boron have?
↓↑ ↓↑ ↓
Has: 2 pairs and 1 unpaired electron
1𝑠 2𝑠 2𝑝
21. How many paired and unpaired D electrons does Cobalt have?
↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓↑ ↓ ↓ ↓
Has: 2 pairs and 3 unpaired D electron
1𝑠 2𝑠
2𝑝
3𝑠
3𝑝
4𝑠
3𝑑
22. Give the electron configuration for a neutral atom of beryllium.1s2 2s2
23. Give the electron configuration for a neutral atom of chlorine.1s2 2s2 2p6 3s2 3p5
24. Write the electron configuration for chromium.1s2 2s2 2p6 3s2 3p64s2 3d4
25. What is the electron configuration of oxygen?1s2 2s2 2p4
26. What is the electron configuration of sulfur?1s2 2s2 2p6 3s2 3p64s2 3d4
27. Give the electron configuration for calcium the ion.1s2 2s2 2p6 3s2 3p64s2 (it has lost 2 e-)
28. Give the electron configuration for the oxygen ion.1s2 2s2 2p6 3s2 3p6 (it has gained 2 e-)
29. Give the electron configurations for iodine and its 1– ion.
I neutral:[Kr] 5s2, 4d105p5 ,
I ion: [Kr] 5s2, 4d10 5p6 (it has gained 1 e-)
30. Give the electron configuration for the chloride ion.1s2 2s2 2p6 3s2 3p6 (it has gained 1 e-)
31. How many electrons are in the third energy level of Nickel?1s2 2s2 2p6 3s2 3p64s2 3d8 has 16 e- in 3rd
level
32. How many electrons are in the second energy level of Argon?1s2 2s2 2p6 3s2 3p6 has 8 e- in 3rd level
Average Atomic Mass
you MUST show your work to receive full credit!!
33. What is average atomic mass of Lithium if 7.42% exists as Li-6 and 92.58% exists as Li-7)?
0.0742 x 6 + 0.9258 x 7 = 6.9258 = 6.93 (sigfigs)
34. Magnesium has three naturally occurring isotopes. 78.70% of Magnesium atoms exist as Magnesium-24 ,
10.03% exist as Magnesium-25, and 11.17% exist as Magnesium-26 . What is the average atomic mass
of Magnesium? 0.7870 x 24 + 0.1003 x 25 + 0.1117 x 26 = 24.2997= 24.30 (sigfigs)
35. Neon has two major isotopes, Neon-20 and Neon-22. Out of every 250 neon atoms, 90.0% will be Neon20, and 10.0% will be Neon-22. What is the average atomic mass of Neon?
0.900 x 20 + 0.100 x 22 = 20.2
Periodic Table and Trends
36. What is the name of the following groups
a. Group 1: alkali metals
b. Group 2: alkaline earth metals
c. Group 17: halogens
d. Group 18: noble gases
e. D- block: transition metals
f. F-block : inner-transition metals
37. How are the elements arranged on the periodic table?By increasing atomic number
38. Why do element in the same family have similar chemical properties?b/c they have the same number of
valance electrons
39. What type of elements is found in the upper right hand part of the periodic table?nonmetals
40. What type of elements is found in the lower left hand part of the periodic table?metals
41. Where are metalloids found on the periodic table?Along the dark (or red) stair case line
42. From which orbital in a lithium atom is an electron transferred to form Li ion? Looses electrons from 2s
43. What orbital is filled when iodine gains an electron to become a negative ion? Gaines electrons to the 5p
44. In which group in the periodic table do the elements have the highest electronegativity values? Halogens
(noble gas has zero electronegativity cause they generally don’t form bonds)
45. How many electrons are in the highest occupied energy level of a neutral strontium atom? 2 valance
electrons
46. How many electrons are in the highest occupied energy level of copper? 2 valance electrons (d electrons
are in lower energy level)
47. How many electrons are present in the d sublevel of a neutral atom of nickel? 8 electrons in 3 d sublevel
48. The ionization energy of elements _increase_ as you go from left to right and _decrease_ as you go from
top to bottom.
49. The electronegativity of elements _increase_ as you go from left to right and _decrease_ as you go from
top to bottom.
50. The atomic radius of elements _decrease_ as you go from left to right
51. Why does the radius do this? Because of an increase in affective nuclear charge
52. The atomic radius of element _increase_ as you go from top to bottom.
53. Why does the radius do this? Because of the addition of energy levels
54. The ionic radius of elements decrease as you go from left to right and increase as you go from top to
bottom
55. Circle the element in each group that has the highest Electronegativity.
g. Na, Fr, Rb
b. Mo, I , K
c. F, Se, Mg
56. Circle the element in each group that has the highest ionization energy
a. Na, Fr, Rb
b. Mo, I , K
c. F, Se, Mg