Download Unit 3 Test Review – Periodic Table (Yes, this is worth a grade!) Fill

Unit 3 Test Review – Periodic Table (Yes, this is worth a grade!)
Fill in the missing information on the table
Element
Atomic Symbol
# of Valence
Electrons
Lewis Dot Structure
Charge
Bromine
Xenon
How many valence electrons do the following elements have?
Sr________
P_______
Li________
N________
Xe_________
What is the most likely charge of each element below when they ionize?
N_______
K________
Kr________
Ca_________
Br_________
Match the following terms with their definitions
1. _____ Atomic Radius
A. the energy required to remove an electron from a
gaseous atom or ion.
2. _____ Ion
B. atom which has gained or lost valance electrons
and thus gained an overall positive or negative charge.
3. _____ Electronegativity
C. measure of the attraction of an atom for the
electrons in a chemical bond.
4. _____ Ionization Energy
D. approximately the measure of the distance from
the center of an atom to the outermost electron
cloud.
Fill in the Blank (Increases or Decreases)
1. As you go across the periodic table from left to right, ionization energy __________________
2. As you go across the periodic table left to right, atomic size ___________________
3. As you go across the periodic table right to left, electronegativity ___________________
4. As you go down the periodic table, atomic size ___________________
5. As you go down the periodic table, electronegativity ___________________
6. As you go up the periodic table, ionization energy _________________
Determine whether element is likely to GAIN electrons (become a “-“ ion) or LOSE electrons (become a “+”
ion) and determine how many electrons would be gained/lost.
1. Nitrogen (N)
2. Astatine (At)
3. Cesium (Cs)
5. Calcium (Ca)
4. Fluorine (F)
Use the periodic table to arrange the atoms from largest to smallest in atomic size.
1. P , Sb , N , Bi ___________________________________________
2. Zn , K , Fe , Br __________________________________________
3. W , Au , Ta , Cs _________________________________________
4. Mg , Sr , Ca , Ra _________________________________________
Which atom in each of the following pairs would have the higher first ionization energy?
1. K , Li __________
2. P , S __________
3. F , I __________
In each of the following pairs of particles, pick the atom or ion that is larger.
4. S2- , S __________
5. Al , Al3+ __________
6. Se2- , O2- __________
Rank the following in order of INCREASING (smallest to largest) electronegativity
7. Be , C , Li , O ________________________________________________
8. P , Sb , N , Bi ________________________________________________
9. P , As , N , Bi ________________________________________________
10. Zn , K , Fe , Br ________________________________________________
Multiple Choice Practice Problems
1. In the modern periodic table, elements are ordered
A) according to decreasing atomic mass
B) according to Mendeleev’s original design
C) according to increasing atomic number
D) based on when they were discovered
2. Lithium and potassium are ____ based on their positions on the periodic table.
A) alkali metals
B) transition metals
C) halogens
D) noble gases
3. Fluorine and chlorine are ____ based on their positions on the periodic table.
A) alkaline-earth metals
C) halogens
B) transition elements actinides
D) noble gases
4. The energy it takes to attract an electron from an atom _____ as you move across a
period.
A) generally increases
C) generally decreases
B) does not change
D) varies unpredictably
Use the diagram to answer questions 5-6.
5. Which general trend exists for ionization energy across a period?
A) Ionization energy increases
B) Ionization remains fairly constant.
C) Ionization energy decreases
D) Ionization energy first increases then decreases
6. Which of the following statements correctly explains why the ionization energy of atoms decreases as you
move from top to bottom in the alkali metals?
A) Valence electrons are attracted more to atoms containing a lot of protons.
B) Valence electrons in larger atoms are more loosely held.
C) Atoms with fewer protons will lose electrons easily.
D) Atoms with more protons will lose electrons easily.
7. Which group tends to have the highest ionization energy? The lowest?
A) halogens; alkaline earth metals
C) alkali metals; noble gases
B) alkaline earth metals; halogens
D) noble gases; alkali metals
8. Which of the following statements regarding ionization energy is true?
A) Periodic trends in ionization energies are opposite those for atomic size.
B) Periodic trends in ionization energies are opposite those for electronegativity.
C) Periodic trends in ionization energies are opposite those for electron affinity.
D) none of the above
9. The elements in the modern periodic table are arranged by increasing
A) density
B) size
C) atomic mass
D) atomic number
10. Elements in the same family have similar chemical properties because
A) they have the similar atomic masses
B) their electron arrangement is similar
C) they are the same size
D) none of these
11. Which of the following is not a property of a metal?
A) they react with acids
B) they are malleable
C) they conduct electricity
D) they form negative ions
12. Which element has properties that most resemble argon?
A) oxygen
B) xenon
C) iodine
D) zinc
Match the element to the description in questions 13 - 26.
_____ 13. alkaline earth metal
a. silver
_____ 14. alkali metal
b. magnesium
_____ 15. noble gases
c. chlorine
_____ 16. halogens
d. sodium
_____ 17. transition metal
e. neon
_____ 18. a highly reactive, greenish-yellow gas
used as a bleach and water disinfectant
_____ 19. best conductor of heat and electricity.
_____ 20. has a completely filled outer energy level
_____ 21. used in advertising signs
_____ 22. forms table salt when combined with chlorine
_____ 23. used for coins, fine eating utensils and jewelry
_____ 24. has 1 valance electron
_____ 25. unreactive
_____ 26. has 2 valence electrons