Periodic Trends Test Review
1. Horizontal rows on the periodic table are called
a. groups
b. classes
c. families
d. periods
2. Mendeleev organized the periodic table according to
a. atomic number
b. atomic mass
c. molar mass
d. nuclear charge
3. Alkali metals
a. are highly reactive
b. can be cut with a knife
c. have 1 valence electron
d. all of the above
4. An example of a metalloid is
a. Silicon
b. Phosphorus
c. Selenium
d. Bromine
5. Which element has 7 valence electrons
a. Manganese
b. Iodine
c. Krypton
d. Sulfur
6. What is an electrons valence shell?
a. the number of electrons an element has
b. the outermost energy level
c. the electrons effective nuclear charge
d. the 5th energy level
7. Group 17 elements are known as
a. alkali metals
b. alkaline earth metals
c. noble gases
d. halogens
8. An anion is a
a. positive ion
b. negative ion
c. neutron
d. neutral element
9. Argon is an example of
a. noble gas
b. halogen
c. metalloid
d. metal
10. How many valence electrons does Aluminum have?
a. 5
b. 13
c. 3
d. 4
11. Where are non-metals found on the periodic table?
a. left
b. right
c. between metals and metalloids
d. scattered throughout the periodic table
12. Columns on the periodic table are known as
a. periods
b. classes
c. sections
d. groups
13. To which Family or Group do Ca and Ba belong?
a. alkali metals
b. halogens
c. alkaline earth metals
d. noble gases
14. Which of the following is NOT a characteristic of a metal?
a. malleable
b. ductile
c. semi-conductor
d. mostly solid at room temperature
15. Periodic law states
a. physical properties of elements are functions of their atomic number
b. chemical properties of elements are functions of their atomic number
c. both a and b
d. none of the above
16. Which element has the smallest atomic radius?
a. Cesium (Cs)
b. Hafnium (Hf)
c. Gold (Au)
d. Mercury (Hg)
17. Which element has the highest electron affinity?
a. Carbon
b. Fluorine
c. Oxygen
d. Lithium
18. How many energy levels does Ca have?
a. 1
b. 2
c. 3
d. 4
19. An element that gains an electron becomes
a. a cation
b. an anion
c. an isotope
d. neutron
20. Which of the following elements would most likely become a cation?
a. Potassium
b. Aluminum
c. Chlorine
d. Fluorine
21.An ion is an element that has
a. gained an electron
b. lost an electron
c. a neutral charge
d. gained or lost an electron
22. As ENC increases
a. electron affinity increases
b. electronegativity increases
c. ionization energy increase
d. all of the above
23. Effective nuclear charge is approximately equal to
a. the number of electrons an element has
b. the number of valence electrons an element has
c. the number of energy levels an element has
d. the ionization energy
24. Atomic Radius is highest on the periodic table
a. the bottom left
b. the bottom right
c. the top left
d. the top right
25. Which of the following elements has the highest 1st ionization energy
a. Lithium
b. Potassium
c. Neon
d. Fluorine
26. Which of the following elements is the least electronegative
a. Carbon
b. Nitrogen
c. Bromine
d. Sulfur
27. A cation is always
a. larger
b. smaller
c. equal to in size
d. double
than the element from which it was formed
28. An electron that is available to be lost, gained or shared is called
a. ground state electron
b. valence electron
c. valence shell
d. electronegative
29. Which element would be most like Iron in physical and chemical properties
a. Ruthenium
b. Nickel
c. Calcium
d. Iridium
30. Which of the following elements has the largest atomic radius
a. Magnesium
b. Chlorine
c. Rubidium
d. Phosphorus
31. How many valence electrons does He have?
a. 8
b. 2
c. 1
d. 4
32. Whose work led to the recognition that atomic number not atomic mass is the basis for the organization of the periodic
table?
a. Mendeleev
b. Rutherford
c. Bohr
d. Moseley
33. Electronegativity is
a. the ability of an atom to give away electrons
b. the ability of an atom to gain electrons
c. the ability of an atom to remain neutral
d. the ability of an atom to become and ion
34. Which isotope of Carbon would be most common?
a. Carbon -14
b. Carbon -12
c. Carbon -11
d. Carbon -6
35. What is the molar mass of I2?
a. 126.90 g
b. 126.90 amu
c. 253.80 g
d. 253.80 amu
36. Explain your answer for question 29.
37. What is the most common isotope of Boron?
38. List 2 differences between metals, non-metals and metalloids
39. How many moles of Sodium Bicarbonate in 145 g NaHCO3?
40. Explain why the first ionization energy of Magnesium is higher than that of Lithium.
41. Explain why the 2nd ionization energy of Lithium is higher than that of Magnesium.
42. How many moles are there in 3.00g of boron tribromide, BBr3?
43. How many chlorine atoms in 58.21 g of MgCl2?
44. Put the following in order from highest to lowest Ionization Energy – O, Ca, Li, S.
45. Put the following in order from lowest to highest Electronegativity – Al, Cl, Rb, Li.
46. Put the following ions in order of size from smallest to largest – F-, Li+, Cl-, Be+2
47. How many electrons in 1.5 mols of C6H12O6? (extra credit type of question)
48. What type of ion would Aluminum form? Why?
49. What type of ion would Sulfur form? Why?
50. What type of ion would Silicon form? Why?
Answer Sheet
1.d
2.b
3.d
4.a
5.b
6.b
7.d
8.b
9.a
10.c
11.b
12.d
13.c
14.c
15.c
16.d
17.b
18.d
19.b
20.a
21.d
22.d
23.b
24.a
25.c
26.a
27.b
28 b
29.a
30.c
31.b
32.d
33.b
34.b
35.d
36. Ruthenium would be most like Iron in properties because it is in the same family.
37.Boron-11
Boron’s atomic mass (average mass) is 10.811, the closest isotope, and therefore most common, is 11.
38.
Metals-malleable, ductile, high tensile strength, good conductor
Metalloid- medium level of malleability, ductile and tensile strength, semi-conductor
Non-metal-not malleable nor ductile, low tensile strength, poor conductor
39. 145 g NaHCO3 (1 mol NaHCO3/ 84.01 g NaHCO3) = 1.73 mol NaHCO3
40. Because Magnesium has a higher ENC so it holds the electrons tighter. If the electrons are tighter, it takes
more energy to remove one
41. Taking the 2nd electron from Lithium means reaching down into the next energy level, making it much
harder to take that electron
42. 3g BBr3 x (1 mol/ 250.51g BBr3) = 0.012 mol BBr3
43. 58.21 g MgCl2(1 mol MgCl2/95.21g MgCl2)(6.022X1023 molecules MgCl2/mol MgCl2)(2 atoms Cl/1
molecule MgCl2)
7.36 X1023 atoms Cl
(use ENC to determine trends for 44-46)
44. O, S, Ca, Li (O and S are in the same family, so ENC is similar – but stronger at the top)
45. Rb, Li, Al, Cl (Rb and Li are in the same family, so ENC is similar – but weaker at the bottom)
46. Be+2, Li+, F-, Cl47 1.5 mol C6H12O6 (6.022X1023 molecules C6H12O6/1 mol C6H12O6)(96 e-/1 molecule C6H12O6) = 8.67X1025 e6 e- for each C (6*6) + 1 e- for each H (12*1) + 8 e- for each O (6*8) = 96 e48. Aluminum has 3 valence electrons, so it will form a +3 ion (easier to lose 3 electrons than gain 5)
49. Sulfur has 6 valence electrons, so it will form a -2 ion (easier to gain 2 electrons than lose 6)
50. Silicon has 4 valence electrons – so it could lose or gain 4 . . . and instead it likes to share electrons.