Midterm

____ 171. According to the aufbau principle,

a.	an orbital may be occupied by only two electrons.
b.	electrons in the same orbital must have opposite spins.
c.	electrons enter orbitals of highest energy first.
d.	electrons enter orbitals of lowest energy first.

____ 181. How are the frequency and wavelength of light related?

a.	They are inversely proportional to each other.
b.	Frequency equals wavelength divided by the speed of light.
c.	Wavelength is determined by dividing frequency by the speed of light.
d.	They are directly proportional to each other.

____ 182. What is the wavelength of an electromagnetic wave that travels at 3 10 m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)

a.
b.	60 MHz ´ 300,000,000 m/s
c.
d.	No answer can be determined from the information given.

____ 183. The light given off by an electric discharge through sodium vapor is ____.

a.	a continuous spectrum
b.	an emission spectrum
c.	of a single wavelength
d.	white light

____ 184. Emission of light from an atom occurs when an electron

a.	drops from a higher to a lower energy level.
b.	jumps from a lower to a higher energy level.
c.	moves within its atomic orbital.
d.	falls into the nucleus.

____ 185. As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit

a.	increase.
b.	decrease.
c.	remain the same.
d.	cannot be determined.

____ 186. The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be

a.	the same.
b.	different from each other.
c.	the same as those of several other elements.
d.	the same as each other only in the ultraviolet range.

____ 187. What is the approximate energy of a photon having a frequency of 4 10 Hz? (h = 6.6 10 J s)

a.	3 10 J
b.	3 10 J
c.	2 10 J
d.	3 10 J

____ 188. What is the approximate frequency of a photon having an energy 5 10 J? (h = 6.6 10 J s)

a.	8 10 Hz
b.	3 10 Hz
c.	3 10 Hz
d.	1 10 Hz

____ 189. Which variable is directly proportional to frequency?

a.	wavelength
b.	velocity
c.	position
d.	energy

____ 190. How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom?

a.	They are greater in magnitude than those between lower energy levels.
b.	They are smaller in magnitude than those between lower energy levels.
c.	There is no significant difference in the magnitudes of these differences.
d.	No answer can be determined from the information given.

____ 191. What are quanta of light called?

a.	charms
b.	excitons
c.	muons
d.	photons

____ 192. Bohr's model could only explain the spectra of which type of atoms?

a.	single atoms with one electron
b.	bonded atoms with one electron
c.	single atoms with more than one electron
d.	bonded atoms with more than one electron

____ 193. The quantum mechanical model of the atom

a.	defines the exact path of an electron around the nucleus.
b.	was proposed by Niels Bohr.
c.	involves the probability of finding an electron in a certain position.
d.	no longer requires the concept of energy levels.

____ 194. According to the Heisenberg uncertainty principle, if the position of a tiny moving particle is known, the

a.	mass of the particle cannot be exactly determined.
b.	charge of the particle cannot be exactly determined.
c.	spin of the particle cannot be exactly determined.
d.	velocity of the particle cannot be exactly determined.

____ 195. How can the position of a very tiny particle be determined?

a.	by analyzing its interactions with another particle
b.	by measuring its velocity
c.	by measuring its mass
d.	by determining its charge

____ 196. The wavelike properties of electrons are useful in

a.	defining photons.
b.	writing electron configurations.
c.	magnifying objects.
d.	determining the velocity and position of a particle.

____ 197. In an s orbital, the probability of finding an electron a particular distance from the nucleus can best be determined by the

a.	quantum mechanical model.
b.	direction of the electron with respect to the nucleus.
c.	boundary of the electron cloud.
d.	deBroglie equation.

____ 198. What is another name for the representative elements?

a.	Group A elements
b.	Group B elements
c.	Group C elements
d.	transition elements

____ 199. What is another name for the transition metals?

a.	noble gases
b.	Group A elements
c.	Group B elements
d.	Group C elements

____ 200. Which of the following elements is in the same period as phosphorus?

a.	carbon
b.	magnesium
c.	nitrogen
d.	oxygen

____ 201. Each period in the periodic table corresponds to a(n) ____.

a.	principal energy level
b.	energy sublevel
c.	orbital
d.	suborbital

____ 202. The modern periodic table is arranged in order of increasing atomic ____.

a.	mass
b.	charge
c.	number
d.	radius

____ 203. Which of the following categories includes the majority of the elements?

a.	metalloids
b.	liquids
c.	metals
d.	nonmetals

____ 204. Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a.	Pt
b.	V
c.	Li
d.	Kr

____ 205. To what category of elements does an element belong if it is a poor conductor of electricity? ____

a.	transition elements
b.	metalloids
c.	nonmetals
d.	metals

____ 206. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a.	In, 49 protons, 49 electrons
b.	Zn, 30 protons, 60 electrons
c.	Cs, 55 protons, 132.9 electrons
d.	F, 19 protons, 19 electrons

____ 207. The atomic number of an element is the total number of which particles in the nucleus?

a.	neutrons
b.	protons
c.	electrons
d.	protons and electrons

____ 208. What element has the electron configuration 1s2s2p3s3p?

a.	nitrogen
b.	selenium
c.	silicon
d.	silver

____ 209. Which of the following is true about the electron configurations of the noble gases?

a.	The highest occupied s and p sublevels are completely filled.
b.	The highest occupied s and p sublevels are partially filled.
c.	The electrons with the highest energy are in a d sublevel.
d.	The electrons with the highest energy are in an f sublevel.

____ 210. Elements that are characterized by the filling of p orbitals are classified as ____.

a.	groups 3A through 8A
b.	transition metals
c.	inner transition metals
d.	groups 1A and 2A

____ 211. Which of the following electron configurations is most likely to result in an element that is relatively inactive?

a.	a half-filled energy sublevel
b.	a filled energy sublevel
c.	one empty and one filled energy sublevel
d.	a filled highest occupied principal energy level

____ 212. Which subatomic particle plays the greatest part in determining the properties of an element?

a.	proton
b.	electron
c.	neutron
d.	nucleus

____ 213. Which of the following elements is a transition metal?

a.	cesium
b.	copper
c.	tellurium
d.	tin

____ 214. Which of the following groupings contains only representative elements?

a.	Cu, Co, Cd
b.	Ni, Fe, Zn
c.	Al, Mg, Li
d.	Hg, Cr, Ag

____ 215. Which of the following is true about the electron configurations of the representative elements?

a.	The highest occupied s and p sublevels are completely filled.
b.	The highest occupied s and p sublevels are partially filled.
c.	The electrons with the highest energy are in a d sublevel.
d.	The electrons with the highest energy are in an f sublevel.

____ 216. What are the Group 1A and Group 7A elements examples of?

a.	representative elements
b.	transition elements
c.	noble gases
d.	nonmetallic elements

____ 217. Of the elements Fe, Hg, U, and Te, which is a representative element?

a.	Fe
b.	Hg
c.	U
d.	Te

____ 218. How does atomic radius change from top to bottom in a group in the periodic table?

a.	It tends to decrease.
b.	It tends to increase.
c.	It first increases, then decreases.
d.	It first decreases, then increases.

____ 219. How does atomic radius change from left to right across a period in the periodic table?

a.	It tends to decrease.
b.	It tends to increase.
c.	It first increases, then decreases.
d.	It first decreases, then increases.

____ 220. What causes the shielding effect to remain constant across a period?

a.	Electrons are added to the same principal energy level.
b.	Electrons are added to different principal energy levels.
c.	The charge on the nucleus is constant.
d.	The atomic radius increases.

____ 221. Atomic size generally

a.	increases as you move from left to right across a period.
b.	decreases as you move from top to bottom within a group.
c.	remains constant within a period.
d.	decreases as you move from left to right across a period.

____ 222. What element in the second period has the largest atomic radius?

a.	carbon
b.	lithium
c.	potassium
d.	neon

____ 223. Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?

a.	more shielding of the electrons in the highest occupied energy level
b.	an increase in size of the nucleus
c.	an increase in number of protons
d.	fewer electrons in the highest occupied energy level

____ 224. Which of the following elements has the smallest atomic radius?

a.	sulfur
b.	chlorine
c.	selenium
d.	bromine

____ 225. What is the charge of a cation?

a.	a positive charge
b.	no charge
c.	a negative charge
d.	The charge depends on the size of the nucleus.

____ 226. Which of the following statements is true about ions?

a.	Cations form when an atom gains electrons.
b.	Cations form when an atom loses electrons.
c.	Anions form when an atom gains protons.
d.	Anions form when an atom loses protons.

____ 227. The metals in Groups 1A, 2A, and 3A

a.	gain electrons when they form ions.
b.	all form ions with a negative charge.
c.	all have ions with a 1 charge.
d.	lose electrons when they form ions.

____ 228. Which of the following statements is true about ions?

a.	Anions are positively charged ions.
b.	Cations are common among nonmetals.
c.	Charges for ions are always written as numbers followed by a plus or minus sign.
d.	When an anion forms, more electrons are transferred to it.

____ 229. In which of the following sets are the charges given correctly for all the ions?

a.	Na, Mg, Al
b.	K, Sr, O
c.	Rb, Ba, P
d.	N, O, F

____ 230. In which of the following groups of ions are the charges all shown correctly?

a.	Li, O, S
b.	Ca, Al, Br
c.	K, F, Mg
d.	Na, I, Rb

___ 231. What is the element with the lowest electronegativity value?

a.	cesium
b.	helium
c.	calcium
d.	fluorine

____ 232. What is the element with the highest electronegativity value?

a.	cesium
b.	helium
c.	calcium
d.	fluorine

____ 233. Which of the following elements has the smallest ionic radius?

a.	Li
b.	K
c.	O
d.	S

____ 234. What is the energy required to remove an electron from an atom in the gaseous state called?

a.	nuclear energy
b.	ionization energy
c.	shielding energy
d.	electronegative energy

____ 235. By the early 1800’s, chemists started organizing elements into groups because

a.	the printing press made it possible to disseminate knowledge faster.
b.	universities had a sudden influx of students interested in chemistry.
c.	there were so many new elements that had been discovered.
d.	more books were being published on the topic.

____ 236. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?

a.	increase in atomic size (Shielding)
b.	increase in size of the nucleus
c.	increase in number of protons
d.	fewer electrons in the highest occupied energy level

____ 237. Which of the following elements has the smallest first ionization energy?

a.	sodium
b.	calcium
c.	potassium
d.	magnesium

____ 238. Which of the following elements has the lowest electronegativity?

a.	lithium
b.	carbon
c.	bromine
d.	fluorine

____ 239. Which statement is true about electronegativity?

a.	Electronegativity is the ability of an anion to attract another anion.
b.	Electronegativity generally increases as you move from top to bottom within a group.
c.	Electronegativity generally is higher for metals than for nonmetals.
d.	Electronegativity generally increases from left to right across a period.

____ 240. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.

a.	lower
b.	higher
c.	the same
d.	unpredictable

____ 241. Which of the following decreases with increasing atomic number in Group 2A?

a.	shielding effect
b.	ionic size
c.	ionization energy
d.	number of electrons

____ 242. Which of the following statements correctly compares the relative size of an ion to its neutral atom?

a.	The radius of an anion is greater than the radius of its neutral atom.
b.	The radius of an anion is identical to the radius of its neutral atom.
c.	The radius of a cation is greater than the radius of its neutral atom.
d.	The radius of a cation is identical to the radius of its neutral atom.

____ 243. Which of the following factors contributes to the increase in ionization energy from left to right across a period?

a.	an increase in the shielding effect
b.	an increase in the size of the nucleus
c.	an increase in the number of protons
d.	fewer electrons in the highest occupied energy level

____ 244. As you move from left to right across the second period of the periodic table

a.	ionization energy increases.
b.	atomic radii increase.
c.	electronegativity decreases.
d.	atomic mass decreases.

____ 245. Of the following elements, which one has the smallest first ionization energy?

a.	boron
b.	carbon
c.	aluminum
d.	silicon