Download Unit 16 Worksheet - Jensen Chemistry

Name_________________________________________________period____________Unit 16: reaction rates
Review:
1. When do electrons release photons(packets of energy)? When the electrons:
a. move to higher levels of energy
b. return to their original energy level
c increase orbital speed around the nucleus
d. are released by the atom
2. Helium was discovered on the sun in 1868, almost 30 years before it was discovered here on the earth. How could
that be possible?
a. Investigation of light from the sun revealed a spectrum not yet found in known elements.
b. Captured cosmic rays from the sun contained helium.
c. Investigation of the size of solar flares suggested that they consisted of material twice the mass of hydrogen.
d. Meteorites that had traveled through the sun’s atmosphere contained helium.
3. Experiments performed to reveal the structure of atoms led scientists to conclude that an atom’s
a. positive charge is evenly distributed throughout its volume
b. negative charge is mainly concentrated in its nucleus
c. mass is evenly distributed throughout its volume
d. volume is mainly unoccupied
4. As an atom becomes an ion, its mass number
a. decreases
b. increases
c. remains the same
5. What is the nuclear charge of an iron atom?
a. +26
b. +36
c. +56
d. +82
8. What is the molar mass of Ca3(PO4)2?
a. 196 g
b. 214 g
c. 245 g
d. 310 g
9. What is total number of neon atoms contained in 20.2 grams of neon gas?
a. 1.01 x 1024
b. 2.02 x 1024
c. 3.01 x 1023
d. 6.02 x 1023
10. Atoms of metals tend to
a. lose electrons and form negative ions
b. lose electrons and form positive ions
c. gain electrons and form negative ions
d. gain electrons and form positive ions
11. Which of these elements has physical and chemical properties most similar to silicon (Si)?
a. germanium (Ge)
b. silver (Ag)
c. phosphorus (P)
d. chlorine (Cl)
12. The number of neutrons in Antimony 122 is?
a. 51
b. 71
c. 94
d. 122
e. 172
13. All the isotopes of a given atom have:
a. the same atomic mass and the same atomic number
b. the same atomic mass but different atomic numbers
c. different atomic mass but the same atomic number
d. different atomic mass and different atomic numbers
14. What is the structure of a krypton-85 atom?
a. 49 electrons, 49 protons, 85 neutrons
b. 49 electrons, 49 protons, 49 neutrons
c. 36 electrons, 36 protons, 85 neutrons
d. 36 electrons, 36 protons, 49 neutrons
15. Lithium, sodium, potassium, and rubidium are all members of the
a. alkali metals
b. lanthanides
c. halogens
16. Which of the following elements has the strongest attraction for electrons?
a. boron
b. aluminum
c. oxygen
d. sulfur
2+
17. As a Ca atom undergoes oxidation to Ca , the number of neutrons in its nucleus:
a. decreases
b. increases
c. remains the same
18. Which of the following elements would you expect to be an unreactive gas?
a. phosphorus, P
b. calcium, Ca
c. argon, Ar
d. carbon, C
19. As the elements in Group 17 are considered in order of increasing atomic number, the chemical reactivity of each
successive element:
a. decreases
b. increases
20. A characteristic of a nonmetal is
c. remains the same
a. high melting points
b. high electronegativity
c. high electrical conductivity
d. the ability to form positive ions
21. Most of the groups in the Periodic table of the Elements contain
a. nonmetals, only
b. metals, only
c. nonmetals and metals
d. metals and metalloids
22. The proper relationship of wavelength to light energy (E) is:
a. increased wavelength correlates to increased energy
b. increased wavelength correlates to decreased energy
c. wavelength is independent of energy
d. wavelength is independent of frequency
23. What causes the emission of radiant energy that produces characteristic spectral lines?
a. neutron absorption by the nucleus
b. gamma ray emission from the nucleus
c. movement of electrons to higher energy levels
d. return of electrons to lower energy levels
28. How many valence electrons does Si have?
a. one
b. two
c. three
d. four
29. When an atom loses an electron, the atom becomes an ion that is
a. positively charged and gains a small amount of mass
b. positively charged and loses a small amount of mass
c. negatively charged and gains a small amount of mass
d. negatively charged and loses a small amount of mass
30. If M represents a group 1 metal, what is the formula for the compound formed by M and oxygen?
a. MO2
b. M2O
c. M2O3
d. M3O2
31. Which pair of atoms is held together by a covalent bond?
a. HCl
b. LiCl
c. NaCl
d. KCl
32. Which of the following atoms has the greatest tendency to attract electrons?
a. barium
b. beryllium
c. boron
d. bromine
33. Which pair of atoms will share electrons when a bond is formed between them?
a. Ba and I
b. Br and Cl
c. K and Cl
d. Li and I
34. Element X is n Group 2 and element Y is in Group 17. What happens when a compound is formed between these
two atoms?
a. X loses electrons to Y to form an ionic bond.
b. X loses electrons to Y to form a covalent.
c. X gains electrons from Y to form an ionic bond.
d. X gains electrons from Y to form a covalent bond.