Unit 4 Chemistry Review

Valence Electrons

100

Which element is in its ground state? a) Nitrogen (1-6) b) Iron (2-7-15-2 c) Potassium (1-8-9-15) d) Lithium (2-1)

d. Lithium

200

1. How many valence electrons do most atoms need to have a stable configuration? A. 1 B. 6 C. 8 D. 12

C. 8

300

2. What are the only elements that naturally have a stable electron configuration? A. the alkali metals B. the halogens C. the actinides D. the Nobel gases

D. the Nobel gases

400

3. How do atoms get a stable electron configuration if they do not naturally have one? A. by splitting their nucleus B. by chemical bonding C. by adding protons to their nucleus D. by losing neutrons

B. by chemical bonding

500

4. What would a sodium atom have to do in order to get eight valence electrons? A. lose 1 valence electron B. gain 1 valence electron C. lose 7 valence electrons D. gain 3 valence electrons

A. lose 1 valence electron

Octet Rule

100

6. What would an oxygen atom have to do in order to get eight valence electrons? A. lose 2 valence electrons B. gain 2 valence electrons C. lose 3 valence electrons D. gain 3 valence electrons

B. gain 2 valence electrons

200

11. Identify the element in period 2 that contains five electrons in its outermost main energy level. A. beryllium B. carbon C. nitrogen D. oxygen

C. nitrogen

300

14. Among the elements gallium (Ga), bromine (Br), potassium (K), and calcium (Ca), which has the lowest electronegativity? A. Ga B. Br C. K D. Ca

B. Br

400

16. What is the relationship between group number and number of valence electrons in the groups 13-18 (P-Block) elements? A. group number = number of valence electrons B. group number minus 10 = number of valence electrons C. group number = number of valence electrons plus 10 D. group number = number of valence electrons times 8

A. group number = number of valence electrons

500

1) Metals tend to __________ electrons and nonmetals tend to __________ electrons. A) gain, gain B) lose, lose C) lose, gain D) gain, gain E) neither, they keep their electrons

C) lose, gain

Elements and Compund

100

20. Based on electronegativity values, which type of elements tends to have the greatest attraction for electrons in a bond? a. Metals b. Non-metals c. Metalloids d. Noble gases

A. Metals

200

What substance is an element? A. NH3 B. Fe C. C6H1206

Fe

300

A substance that is made of 2 or more elements is called a… A. Solution B. Compound C. Atom

B. Compound

400

A substance that contains only one type of atom is called a… A. Isomer B. Element C. Compound

B. Element

500

Which substance cannot be broken down by a change? Ammonia (NH3) Arsenic (As) Ethane (C2H2)

Arsenic (As)- an ELEMENT

Charge of an ION

100

2) Anions tend to have a __________ charge and cations tend to have a __________ charge. A) positive, positive B) negative, negative C) positive, negative D) negative, positive E) neither, they are both neutral

D) negative, positive

200

4) Which species below is the nitride ion? A) Na+ B) NO3- C) NO2- D) NH4+ E) N3-

E) N3-

300

5) When a metal and a nonmetal react, the __________ tends to lose electrons and the __________ tends to gain electrons. A) metal, metal B) nonmetal, nonmetal C) metal, nonmetal D) nonmetal, metal E) None of the above, these elements share electrons.

C) metal, nonmetal

400

7) Sodium forms an ion with a charge of __________. A) 1+ B) 1- C) 2+ D) 2- E) 0

A) 1+

500

18) Predict the charge of the most stable ion of S A) 3+ B) 1- C) 6+ D) 2+ E) 2-

E) 2-

Atomic Theory

100

What are small, negatively charged particles are called…

Electrons

200

18. Which atom has the lease attraction for the electrons in a chemical bond? a. Helium (He) b. Fluorine (F) c. Silicon (Si) d. Lithium (Li)

a. Helium (He)

300

The Bohr Model states that atoms are…

A. Small, dense ball B. Nucleus surrounded by electrons in different energy levels C. Nucleus surrounded by electrons in orbitals

400

19. Which atom has the greatest attraction for the electrons in a chemical bond? a. Hydrogen (H) b. Fluorine (F) c. Silicon (Si) d. Sulfur (S)

a. Hydrogen (H)

500

21. Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 3 are considered from left to right? a. Both electronegativity and atomic radius increase. b. Both electronegativity and atomic radius decrease. c. Electronegativity increases and atomic radius decreases. d. Electronegativity decreases and atomic radius increases.

c. Electronegativity increases and atomic radius decreases.