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Valence Electrons
Octet Rule
Elements and Compund
Charge of an ION
Atomic Theory
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
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
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
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
100
What are small, negatively charged particles are called…
Electrons
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
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
200
What substance is an element? A. NH3 B. Fe C. C6H1206
Fe
200
4) Which species below is the nitride ion? A) Na+ B) NO3- C) NO2- D) NH4+ E) N3-
E) N3-
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
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
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
300
A substance that is made of 2 or more elements is called a… A. Solution B. Compound C. Atom
B. Compound
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
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
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
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
400
A substance that contains only one type of atom is called a… A. Isomer B. Element C. Compound
B. Element
400
7) Sodium forms an ion with a charge of __________. A) 1+ B) 1- C) 2+ D) 2- E) 0
A) 1+
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
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
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
500
Which substance cannot be broken down by a change? Ammonia (NH3) Arsenic (As) Ethane (C2H2)
Arsenic (As)- an ELEMENT
500
18) Predict the charge of the most stable ion of S A) 3+ B) 1- C) 6+ D) 2+ E) 2-
E) 2-
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.