CHEM 121

Give the atomic symbol of the elements with the following Z value, and classify each as a metal, metalloid, or nonmetal: a) Z = 34; b) Z = 20; c) Z = 29 a. Z = 34 Se nonmetal Z = 20 Ca metal Z = 29 Cu metal b. Z = 34 Se semimetal Z = 20 Ca metal Z = 29 Cu metal c. Z = 34 Se metal Z = 20 Ca metal Z = 29 Cu metal d. Z = 34 Se nonmetal Z = 20 Ne nonmetal Z = 29 Cu metal e. Z = 34 Se nonmetal Z = 20 Ca metal Z = 29 Cu nonmetal

Periodic Table Problem - Know Metals/NM/TM/Metaloids: a. Z = 34 Se nonmetal Z = 20 Ca metal Z = 29 Cu metal

What is the visible wavelength of light?

390-750 nm

An atom of which of the following elements has the largest atomic radius? 1) As 2) Sb 3) P 4) Bi 5) N

4) Bi

Which of the following has the largest radius? 1. Ar 2. Ca2+ 3. Cl- 4. S2- 5. K+

4. S2-

How many electrons can be described by the quantum numbers n = 3, l = 3, ml = 1? A. 0 B. 2 C. 6 D. 10 E. 14

A. 0

How many f orbitals have the value n = 2? A. 0 B. 3 C. 5 D. 7 E. 1

A. 0

Mendeleev is given the most credit for the concept of a periodic table of the elements because: A. He emphasized its usefulness in predicting the existence and properties of unknown elements. B. He grouped elements into triads of similar properties. C. His periodic table was arranged in octaves. D. He had the longest history of research in elemental properties. E. His representation of the table was the most understandable.

A. He emphasized its usefulness in predicting the existence and properties of unknown elements.

Which one of the following substances is classified as an element? A. I2 B. NO C. KCl D. C6H12O6 E. CO

A. I2

Which of the following is incorrect? A. The emission spectrum of hydrogen contains a continuum of colors. B. Diffraction produces both constructive and destructive interference. C. All matter displays both particle and wavelike characteristics. D. Niels Bohr developed a quantum model for the hydrogen atom. E. The lowest possible energy state of a molecule or atom is called its ground state.

A. The emission spectrum of hydrogen contains a continuum of colors.

Which one of the following types of radiation has the shortest wavelength, the greatest energy, and the highest frequency? A. Ultraviolet radiation. B. Infrared radiation. C. Visible red light. D. Visible blue light. E. None, because short wavelength is associated with low energy and low frequency, not high energy and high

A. Ultraviolet radiation.

Atomic orbitals developed using quantum mechanics describe what? A. describe regions of space in which one is most likely to find an electron B. describe exact paths for electron motion C. give a description of the atomic structure which is essentially the same as the Bohr model D. allow scientists to calculate an exact volume for the hydrogen atom

A. describe regions of space in which one is most likely to find an electron

A point in the wave function where the amplitude is zero defines: A. the node B. the excited state C. the amplitude of the wave function D. the frequency of radiation E. none of the above

A. the node

An element with the electron configuration [Xe] 6s24f145d7 would belong to which class on the periodic table? A. transition elements B. alkaline earth elements C. halogens D. rare earth elements E. none of the above

A. transition elements

Of the following elements, which has occupied d orbitals in its ground-state neutral atoms? A. Ba B. P C. Ca D. Si E. Cl

A.) Ba

What set of the three figures below illustrates the Law of Multiple Proportions? See Photo

Answer is B Only.

Which of the following sets contains all the true statements in the set below and no false statements? a) the photoelectric effect exhibits a threshhold frequency b) the photoelectric effect occurs with no time lag c) electromagnetic radiation can behave as quanta or packets of energy where each packet of energy is called a photon. a. a) b. b) c. c) d. a) and b) e. a), b) and c)

Answer is e. a), b) and c) a) the photoelectric effect exhibits a threshhold frequency b) the photoelectric effect occurs with no time lag c) electromagnetic radiation can behave as quanta or packets of energy where each packet of energy is called a photon.

Given the following electronic configuration of neutral atoms, identify the element and state the number of unpaired electrons in its ground state. Example: [He]2s1 Answer: Li, 1 (one space between comma and number) Reference: Ref 2-4 - Fill in the Box [Ar]4s13d5

Answer: Cr, 6

What is the l quantum number for a 4p orbital? A. 2 B. 1 C. 0 D. 3 E. more than one of the above

B. 1

If l = 3, how many electrons can be contained in all the possible orbitals? A. 6 B. 14 C. 7 D. 10 E. 5

B. 14

What is the l quantum number for a 4f orbital? A. 0 B. 3 C. 2 D. 1 E. more than one of the above

B. 3

The energy of the light emitted when a hydrogen electron goes from n = 2 to n = 1 is what fraction of its ground-state ionization energy? A. 1/9 B. 3/4 C. 1/2 D. 1/4 E. 1/8

B. 3/4

If n = 2, how many orbitals are possible? A. 3 B. 4 C. 2 D. 8 E. 6

B. 4

When a hydrogen electron makes a transition from n = 3 to n = 1, which of the following statements is true? I. Energy is emitted. II. Energy is absorbed. III. The electron loses energy. IV. The electron gains energy. V. The electron cannot make this transition. A. I, IV B. I, III C. II, III D. II, IV E. V

B. I, III I. Energy is emitted. & III. The electron loses energy.

Consider an atom traveling at 1% of the speed of light. The de Broglie wavelength is found to be 1.46 × 10-3 pm. Which element is this? A. Be B. Zr C. Hg D. Fe E. P

B. Zr

The electron configuration for the barium atom is: A. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 B. [Xe]6s2 C. 1s2 2s2 2p6 3s2 3p6 4s1 D. 1s2 2s2 2p6 3s2 3p6 4s2 E. none of these

B. [Xe]6s2

When a strontium salt is ignited, it burns with a red flame. The frequency of the light given off by this flame is greater than: A. x-rays B. infrared light C. ultraviolet light D. Gamma rays E. yellow light

B. infrared light

When a strontium salt is ignited, it burns with a red flame. The frequency of the light given off by this flame is greater than: A. yellow light B. infrared light C. ultraviolet light D. radio waves E. x-rays

B. infrared light

When ignited, a uranium compound burns with a green flame. The wavelength of the light given off by this flame is greater than that of A. red light B. infrared light C. radio waves D. ultraviolet light E. none of these

B. infrared light

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of...? A. the aufbau principle B. the Pauli exclusion principle C. Hund's Rule D. the periodic law

B. the Pauli exclusion principle

In a given period this group has the element with the largest atomic radius. A. Group 5A B. Group 3A C. Group 1A D. Group 2A E. Group 4A

C. Group 1A

Sodium losing an electron is an ________ process and fluorine losing an electron is an _______ process. a) endothermic, exothermic b) exothermic, endothermic c) endothermic, endothermic d) exothermic, exothermic e) more information needed

C. endothermic, endothermic

Atoms having equal or nearly equal electronegativities are expected to form A. ionic bonds B. polar covalent bonds C. nonpolar covalent bonds D. covalent bonds E. no bonds

C. nonpolar covalent bonds

Which form of electromagnetic radiation has the longest wavelengths? A. gamma rays B. microwaves C. radio waves D. infrared radiation E. x-rays

C. radio waves

Which of the following best describes an orbital? A. space where electrons are unlikely to be found in an atom B. space which may contain electrons, protons, and/or neutrons C. the space in an atom where an electron is most likely to be found D. small, walled spheres that contain electrons E. a single space within an atom that contains all electrons of that atom

C. the space in an atom where an electron is most likely to be found

In an investigation of the electronic absorption spectrum of a particular element, it is found that a photon having λ = 500 nm provides just enough energy to promote an electron from the second quantum level to the third. From this information, we can deduce : A. the energy of the n = 2 level B. the energy of the n = 3 level C. the sum of the energies of n = 2 and n = 3 D. the difference in energies between n = 2 and n = 3 E. all of these

C. the sum of the energies of n = 2 and n = 3

Enter the symbol of the element in the set below that is a metal. For example, H is the symbol of hydrogen. bromine, calcium, sulfur

Ca

Which of the following statements best describes the Heisenberg uncertainty principle? A. It is impossible to accurately know both the exact location and momentum of a particle. B. The location and momentum of a macroscopic object are not known with certainty. C. The location and momentum of a particle can be determined accurately, but not the identity of the particle. D. The velocity of a particle can only be estimated. E. The exact position of an electron is always uncertain.

Correct: A.) It is impossible to accurately know both the exact location and momentum of a particle.

Elements with _______________ first ionization energies and ___________ electron affinities generally form anions. A) low, very negative B) high, positive or slightly negative C) low, positive or slightly negative D) high, very negative E) None of the above is generally correct.

D) high, very negative

Which one of the following substances is not a chemical compound? A. H2S B. Co C. HF D. NO E. HF

D. Co It is a single element.

Which of the following statements is (are) true? I. An excited atom can return to its ground state by absorbing electromagnetic radiation. II. The energy of an atom is increased when electromagnetic radiation is emitted from it. III. The energy of electromagnetic radiation increases as its frequency increases. IV. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appropriate frequency. V. The frequency and wavelength of electromagnetic radiation are inversely proportional to each other. A. II, III, IV B. III, V C. I, II, III D. III, IV, V E. I, II, IV

D. III, IV, V III. The energy of electromagnetic radiation increases as its frequency increases. IV. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appropriate frequency. V. The frequency and wavelength of electromagnetic radiation are inversely proportional to each other.

The first scientist to show that atoms emit any negative particles was:

D. J. J. Thomson Bonus Info: J.J. Thomson was able to measure the charge to mass ratio of the electron; he could not however, measure accurately the charge or mass independently. Thomson (1856-1940) discovered the "electron" in a series of experiments designed to study the nature of electric discharge in a high-vacuum cathode-ray tube.

The scientist who discovered the law of conservation of mass and is also called the father of modern chemistry is:

D. Lavoisier

Choose the element with the smallest atomic radius. A. Cs B. Na C. Rb D. Li E. K

D. Li

An element has the electron configuration [Kr] 5s24d105p2. The element is a(n) A. lanthanide B. nonmetal C. transition element D. metal E. actinide

D. metal Watch this one

Generally, observed behavior that can be formulated into a statement, sometimes mathematical in nature, is called a(n) A. observation B. measurement C. hypothesis D. natural law E. experiment

D. natural law Natural laws summarize patterns that recur in a large amount of data. Unlike human laws, natural laws don't forbid or permit; they describe.

From the following list of observations, choose the one that most clearly supports the following conclusion: a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Electromagnetic radiation has wave characteristics. A. observation a B. observation b C. observation c D. observation d E. observation e

D. observation d

From the following list of observations, choose the one that most clearly supports the following conclusion: a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Spacing between atoms in a crystal is on the same order as the de Broglie wavelength of accelerated electrons. A. observation a B. observation b C. observation c D. observation d E. observation e

D. observation d

How many of the following electron configurations for the species in their ground state are correct? See Picture 1) Ca : 1s2 2s2 2p6 3s2 3p6 4s2 2) Mg: 1s2 2s2 2p6 3s1 3) V : [Ar]3s2 3d3 4) As: [Ar]4s2 3d10 4p3 5) P : 1s2 2s2 2p6 3p5

E. 2 are correct Ca : 1s2 2s2 2p6 3s2 3p6 4s2 or [Ar]4s2 As: [Ar]4s2 3d10 4p3

The number of orbitals in a subshell having a given value of l is equal to: A. l + ml B. 3l C. the number of lobes in each orbital D. 2n + 2 E. 2l + 1

E. 2l + 1

Consider the following representation of a 2p-orbital (There's a Pic of a Figure 8) Which of the following statements best describes the movement of electrons in a p-orbital? A. The electrons move along the outer surface of the p-orbital, similar to a "figure 8" type of movement. B. The electrons move within the two lobes of the p-orbital, but never beyond the outside surface of the orbital. C. The electrons are concentrated at the center (node) of the two lobes. D. The electrons are only moving in one lobe at any given time. E. The electron movement cannot be exactly determined.

E. The electron movement cannot be exactly determined.

The statement "The total mass of materials is not affected by a chemical change in those materials" is called a(n) A. theory B. measurement C. observation D. experiment E. natural law

E. natural law

Which subatomic particle was found to be present in cathode rays? Type its name only in the box.

Exact Match: electrons

Which of the following exhibits the correct orders for both atomic radius and ionization energy, respectively? (smallest to largest) A. S, O, F, and F, O, S B. F, S, O, and O, S, F C. S, F, O, and S, F, O D. F, O, S, and S, O, F E. none of these

F, O, S,and S,O, F

T or F: A chemical theory that has been known for a long time becomes a law.

False

T or F: All matter exhibits either particulate or wave properties exclusively.

False

T or F: Bohr's model correctly describes the hydrogen atom and other small atoms.

False

T or F: The SI unit for frequency is cycles per second.

False

T or F: Bohr's model correctly describes the hydrogen atom and other small atoms.

False Hydrogen only

T or F: The number of neutrons in an atom is the same for all neutral atoms of that element.

False -- Think Isotopes. Neutral is about the Electron/Proton Balance.

Who proposed the principle which states that one cannot simultaneously know the exact position and velocity of a particle?

Heisenberg

Choose the atom or ion using a periodic table. Larger first ionization energy, C or N Fill In Blank

N

An atom of which of the following elements has the largest atomic radius? Cl P Na S Si

Na

Choose the atom or ion using a periodic table. Larger first ionization energy, Na or Rb

Na

Choose the element with the smallest atomic radius. A. Li B. Cs C. Na D. Rb E. K

Need Answer

A specific wave function is called a(n) __________. Fill in the Blank

Orbital

T or F: A gamma ray of wavelength 1.00 × 10-8 cm has enough energy to remove an electron from a hydrogen atom.

True

T or F: Diffraction results when light is scattered from a regular array of points or lines.

True

T or F: The Lewis structure for CHCl3 has nine lone electron pairs.

True

T or F: The magnetic quantum number is related to the orientation of the orbital in space relative to the other orbitals in the atom.

True

T or F: The size of an orbital is arbitrarily defined.

True

Nitrogen has five valence electrons. Consider the following electron arrangements. See Pic in Answer: "x" just means blank (placeholder) Which represents the ground state for N? 2s 2p a) ↑↓ ↑ ↑ ↑ b) ↑ ↑↓ ↑ ↓ c) ↑ ↑↑ ↑ ↑ d) ↑↓ ↑ ↑ x e) ↑↓ ↑↓ ↑ ↑ Reference: 2 - 3

Which represents the ground state for N? Correct Answer is D. for option a See Picture.

Identify the mass law that each of the following observations demonstrates, and explain your reasoning: a) A sample of potassium Chloride from Chile contains the same percent by mass of potassium as one from Poland b) A flashbulb contains magnesium and oxygen before use and magnesium oxide afterward, but its mass does not change. c) Arsenic and oxygen form one compound that is 65.2 mass % arsenic and another that is 75.8 mass % arsenic.

a) Law of Definite Composition — The compound potassium chloride, KCl, is composed of the same elements and same fraction by mass, regardless of its source (Chile or Poland). b) Law of Mass Conservation — The mass of the substance inside the flashbulb did not change during the chemical reaction (formation of magnesium oxide from magnesium and oxygen). c) Law of Multiple Proportions — Two elements, O and As, can combine to form two different compounds that have different proportions of As present.

Which of the following covalent bonds has the highest percent ionic character? a. C - O b. C - Cl c. C - C d. C - H e. N - C

a. C - O

Calculate the lattice energy of magnesium sulfide from the data given below. Mg(s) → Mg(g) ∆H° = 148 kJ/mol Mg(g) → Mg2+(g) + 2e¯ ∆H° = 2186 kJ/mol S8(s) → 8S(g) ∆H° = 2232 kJ/mol S(g) + 2e¯ → S2¯(g) ∆H° = 450 kJ/mol 8Mg(s) + S8(s) → 8MgS(s) ∆H° = -2744 kJ/mol Mg2+(g) + S2¯(g) → MgS(s) ∆H°lattice = ? a. -3406 kJ/mol b. -2720. kJ/mol c. 2720. kJ/mol d. 3406 kJ/mol e. None of these choices is correct.

a. -3406 kJ/mol

Which statement is NOT true of Bohr's model of the atom? a. Bohr's model correctly described the atomic spectra of H and He but failed for other atoms b. An electron does not radiate energy while in a stationary state. c. An electron can move to a different orbit only by absorbing or emitting a photon. d.The energy of a photon absorbed or emitted by an electron is equal to the difference between two energy states. e. Electrons in stationary states in the Bohr hydrogen atom occupied circular orbits.

a. Bohr's model correctly described the atomic spectra of H and He but failed for other atoms

Which of the following bonds has the lowest percent ionic character? a. C-H b. Na-I c. H-F d. K-F e. Li-Cl

a. C-H

In which atom are the 3s and 3p orbitals equal in energy? a. H b. He c. C d. O e. none of these

a. H

In which atom is the 2s orbital highest (least negative) in energy? a. Li b. Be c. B d. C e. N

a. Li

Which of the following would have the greatest lattice energy? a. MgO b. LiF c. NaCl d. KBr e. CsI

a. MgO

Arrange oxygen, sulfur, calcium, rubidium and potassium in order of decreasing electronegativity. a. O > S > Ca > K > Rb b. O > S > Ca > Rb > K c. O > S > Rb > K > Ca d. O > S > Rb > Ca > K e. None of these choices is correct.

a. O > S > Ca > K > Rb

Which one of the following combinations of names and formulas of ions is incorrect? a. O2- oxide b. Al3+ aluminum c. NO3- nitrate d. PO43- phosphate e. CrO42- chromate

a. O2- oxide

Which of the following has the smallest radius? a. P b. Cl- c. Al d. S2- e. Ga

a. P

What set of the elements below includes just the nonmetals? Ga, P, I, Ra, Li, La, Xe a. P, I, Xe b. P, I, La c. I, Xe, Ra d. Ga, P, Xe, e. P, I, L

a. P, I, Xe

Which of the following elements is the most electronegative? a. S b. Ru c. Si d. Te e. Cs

a. S

Which of the following is NOT a feature of Thompson's "Raisin Pudding" model of the atom? a. The presence of a nucleus b. The electrons are dispersed throughout the atom. c. The positive charges in an atom hold the electrons in place. d. The positive charge is dispersed in a cloud about the atom. e. The size of the atom is not dependent on the number of electrons in the atom.

a. The presence of a nucleus

What keeps the electrons from leaving the atom in the Thompson "Raisin Pudding" model of the atom? a. They are embedded in a spherical cloud of positive charge. b. Nothing stops them from leaving. c. The repulsive forces between electrons d. A membrane on the surface of the cloud of positive charge e. The attractive force between the electrons and the nucleus

a. They are embedded in a spherical cloud of positive charge.

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy. a. radio, infrared, ultraviolet, gamma rays b. radio, ultraviolet, infrared, gamma rays c. gamma rays, infrared, radio, ultraviolet d. gamma rays, ultraviolet, infrared, radio e. infrared, ultraviolet, radio, gamma rays

a. radio, infrared, ultraviolet, gamma rays

In which of the following compounds does the bond between the central atom and bromine have the greatest ionic character? a) LiBr b) KBr c) SeBr2 d) AsBr3 e) CaBr2

b) KBr

Rank the members of this set of compounds in order of decreasing ionic character of their bonds. Use partial charges to indicate the bond polarity of each bond. BF3, NF3, CF4 a. C-F > B-F > N-F δ- δ+ δ- δ+ δ- δ+ b. B-F > C-F > N-F δ+ δ- δ+ δ- δ+ δ- c. N-F > C-F > B-F δ+ δ- δ+ δ- δ+ δ- d. N-F > B-F > C-F δ- δ+ δ- δ+ δ- δ+ e. none of these

b. B-F > C-F > N-F δ+ δ- δ+ δ- δ+ δ-

In a Millikan oil-drop experiment, the charges on several different oil drops were as follows: -5.92; -4.44; -2.96; -8.88. The units are arbitrary. What is the likely value of the electronic charge in these arbitrary units? a. -1.11 b. -1.48 c. -2.22 d. -2.96 e. -5.55

b. -1.48 Why?

Which of the following is a nonmetal? a. Ca b. Br c. Fe d. Sb e. Ho

b. Br

What is the identity of element E if the ion E 1- contains 18 electrons?

b. Cl

How many electrons are present in the Be^2+ a. 4 b. 6 c. 2 d. 9 e. 7

c. 2

Determine the number of unpaired electrons in ground state atoms of P and Cl, respectively. a. 5, 3 b. 5, 1 c. 3, 1 d. 3, 2 e. 3, 5

c. 3, 1

Which of the following is NOT a true statement concerning energy levels in atoms? a. In high numbered shells of a multielectron atom, some subshells of different shells have nearly identical energies. b. In the hydrogen atom, all subshells of a given shell have the same energy. c. In a multielectron atom, the various subshells of a given shell have different energies. d. Orbital energies are usually different in multielectron atoms than the corresponding ones in the hydrogen atom. e. The orbitals within a subshell of a multielectron atom have different energies.

e. The orbitals within a subshell of a multielectron atom have different energies.

What component of atoms was discovered by Rutherford? Type its name only in the box.

nucleus

An atom of which of the following elements has the largest atomic radius? 1) Ge 2) K 3) Cl 4) Ca 5) As

1) K

Indicate the charge on the sulfide ion. 1. 2- 2. 3- 3. 1- 4. 4- 5. 2+

1. 2-

The number of unpaired electrons in a nitrogen atom is 1. 3 2. 1 3. 5 4. 2 5. 4

1. 3

When moving down a group (family) in the periodic table, the number of valence electrons 1. remains constant 2. changes in an unpredictable manner 3. decreases regularly 4. doubles with each move 5. increases by 2 then 8 then 18 then 32

1. remains constant

From the following list of observations, choose the one that most clearly supports the following conclusion: a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Electrons in atoms have quantized energies. A. observation a B. observation b C. observation c D. observation d E. observation e

A. observation a

A point in the wave function where the amplitude is zero defines A. the node B. the excited state C. the amplitude of the wave function D. the frequency of radiation E. none of the above

A. the node

How many of the following is/are INCORRECT? i. The importance of the equation E = mc2 is that energy has mass. ii. Electromagnetic radiation can be thought of as a stream of particles called photons. iii. Electromagnetic radiation exhibits wave properties. iv. Energy can only occur in discrete units called quanta. A. 0 B. 1 C. 2 D. 3 E. 4

A. 0

The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 × 10-7 m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li2+ ion? A. 1/9 B. 1/7 C. 1/4 D. 1/3 E. 1

A. 1/9

Which of the following is an incorrect designation for an atomic orbital? A. 1p B. 6s C. 4f D. 1s E. 3d

A. 1p

The electron configuration for the carbon atom is: A. 1s2 2s2 2p2 B. [He]2s4 C. [Ne]2s22p2 D. 1s22p4 E. none of these

A. 1s2 2s2 2p2

Consider the following two compounds: H2O and H2O2. According to the law of multiple proportions, the ratio of hydrogen atoms per gram of oxygen in H2O to hydrogen atoms per gram of oxygen in H2O2 is A. 2:1 B. 4:1 C. 2:2 D. 1:1 E. 1:2

A. 2:1

The number of orbitals having a given value of l is equal to: A. 2l + 1 B. 2n + 2 C. 3l D. l + ml E. the number of lobes in each orbital

A. 2l + 1

The energy of the light emitted when a hydrogen electron goes from n = 2 to n = 1 is what fraction of its ground-state ionization energy? A. 3/4 B. 1/2 C. 1/4 D. 1/8 E. 1/9

A. 3/4

If the Thomson model of the atom had been correct, Rutherford would have observed: A. Alpha particles going through the foil with little or no deflection. B. Alpha particles greatly deflected by the metal foil. C. Alpha particles bouncing off the foil. D. Positive particles formed in the foil. E. None of the above observations is consistent with the Thomson model of the atom.

A. Alpha particles going through the foil with little or no deflection.

An element E has the electron configuration: [Kr] 5s2 4d10 5p2. The formula for the fluoride of E is most likely: See Picture for clarity. A. EF4 B. EF6 C. EF14 D. EF E. EF8

A. EF4 Best Answer: look at the number of valence electron here. it's on the orbital number 5, having a total of 4 valence electrons (outermost shell electrons) that will contribute to bonding. So with F having a -1 charge. And E will have to be a cation of +4. So total is EF4.

Consider the following orderings. I. Na+ < Mg2+ < Al3+ < Si4+ II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Al < Si < P < Cl Which of these give(s) a correct trend in ionization energy? A. I, III, IV B. II, IV C. none of them D. III E. I, IV

A. I, III, IV Need to Study This

Which of the following species is best described by drawing resonance structures? A. O3 B. HCN C. NH4+ D. PH3 E. SO3

A. O3

Of the following elements, which needs three electrons to complete its valence shell? A. P B. Si C. Ba D. Ca E. Cl

A. P

Who was the first scientist to propose that an object could emit only certain amounts of energy? A. Planck B. Einstein C. Bohr D. Rydberg E. de Broglie

A. Planck

Which of the following concerning second ionization energies is true? A. That of Al is higher than that of Mg because the electrons are taken from the same energy level, but the Al atom has one more proton. B. That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to take the second electron away. C. That of Al is lower than that of Mg because Mg wants to lose the second electron, thus the energy change is greater. D. That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital, thus it is easier to take. E. The second ionization energies are equal for Al and Mg.

A. That of Al is higher than that of Mg because the electrons are taken from the same energy level, but the Al atom has one more proton.

Consider the ionization energy (IE) of the magnesium atom. Which of the following is not true? Note: Similar question - But Not Exact Letter Choice A. The IE of Mg is lower than that of sodium. B. The IE of Mg is lower than that of Mg+. C. The IE of Mg is higher than that of calcium. D. The IE of Mg is lower than that of neon. E. The IE of Mg is lower than that of beryllium.

A. The IE of Mg is lower than that of sodium.

Many classic experiments have given us indirect evidence of the nature of the atom. Which of the experiments listed below did NOT give the results described? a. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct b. All of the above experiments gave the results described c. Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron d. The electric discharge tube proved that electrons have a negative charge e. The Rutherford experiment was useful in determining the nuclear charge on the atom

A. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct.

Consider the following portion of the energy-level diagram for hydrogen: n = 4 -0.1361 × 10-18 J n = 3 -0.2420 × 10-18 J n = 2 -0.5445 × 10-18 J n = 1 -2.178 × 10-18 J For which of the following transitions does the light emitted have the longest wavelength? A. n = 4 to n = 3 B. n = 4 to n = 2 C. n = 4 to n = 1 D. n = 3 to n = 2 E. n = 2 to n = 1

A. n = 4 to n = 3

What is the identity of element Q if the ion Q2- contains 36 electrons? Type the correct symbol for the element in the box:

Answer: Se This element is up 2 electrons, so you look for the element with 34 protons.

T or F: A gamma ray of wavelength 1.00 × 10-8 cm has enough energy to remove an electron from a hydrogen atom.

Answer: True

The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is: A. William Thomson B. Ernest Rutherford C. J. J. Thomson D. John Dalton E. Lord Kelvin

B. Ernest Rutherford

T or F: Because Li is the strongest reducing agent of the alkali metals, it reacts most quickly with water of the alkali metals.

False -- Don't know why yet?

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects? A) Larger nuclear charge lowers energy, more electrons in an orbital lowers energy. B) Larger nuclear charge lowers energy, more electrons in an orbital increases energy. C) Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy. D) Smaller nuclear charge lowers energy, more electrons in an orbital increases energy. E) None of the above statements is generally correct.

B) Larger nuclear charge lowers energy, more electrons in an orbital increases energy.

Which inventor/discovery is mismatched in the following list? A) Lavoisier—Law of Conservation of Mass B) Proust—mass of an electron C) Dalton—Atomic Theory of Matter D) Mendeleev—Periodic Table E) Arrhenius—acids produce H+

B) Proust—mass of an electron

Which word best describes the phenomenon which gives rise to a rainbow? A) reflection B) dispersion C) diffraction D) interference E) deflection

B) dispersion

How many d orbitals have n = 3? A. 2 B. 5 C. 10 D. 7 E. 18

B. 5

Avogadro's hypothesis states that: A. Each atom of oxygen is 16 times more massive than an atom of hydrogen. B. At the same temperature and pressure, equal volumes of different gases contain an equal number of particles. C. A given compound always contains exactly the same proportion of elements by mass. D. Mass is neither created nor destroyed in a chemical reaction. E. When two elements form a series of compounds, the ratios of masses that combine with 1 gram of the first element can always be reduced to small whole numbers

B. At the same temperature and pressure, equal volumes of different gases contain an equal number of particles.

Which of the following ionic compounds has the smallest lattice energy (i.e., the lattice energy least favorable to a stable lattice)? A. MgO B. CsI C. LiF D. BaO E. NaCl

B. CsI

Who proposed a model that successfully explained the photoelectric effect? A. Planck B. Einstein C. Compton D. Rydberg E. Bohr

B. Einstein

In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus: A. Energy is emitted. B. Energy is absorbed. C. No change in energy occurs. D. Light is emitted. E. None of these.

B. Energy is absorbed.

Which of the following is a reasonable criticism of the Bohr model of the atom? A. It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. B. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. C. It shows the electrons to exist outside of the nucleus. D. It does not adequately predict the line spectrum of hydrogen. E. It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen.

B. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.

Which of the following best describes an orbital? A. space which may contain electrons, protons, and/or neutrons B. the space in an atom where an electron is most likely to be found C. space where electrons are unlikely to be found in an atom D. a single space within an atom that contains all electrons of that atom E. small, walled spheres that contain electrons

B. the space in an atom where an electron is most likely to be found

Germanium has __________ in its 4p orbitals. A. one electron B. two electrons C. three electrons D. four electrons E. none of these

B. two electrons

Ti has __________ in its d orbitals. A. one electron B. two electrons C. three electrons D. four electrons E. none of these

B. two electrons

Which of the following molecules exhibits the greatest bond energy? A. all the same B. Cl2 C. I2 D. Br2 E. F2

Bond energy (in kJ/mol) F-F:158 Cl-Cl: 244 Br-Br-:193 I-I: 151 Hence, in order of decreasing bond strength: Cl-Cl => Br-Br => (F-F) => I-I Fluorine is an anomaly. Bond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker from chlorine to iodine. Fluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond.

Elements with ________________ first ionization energies and ___________ electron affinities generally form cations. A) low, very negative B) high, positive or slightly negative C) low, positive or slightly negative D) high, very negative E) None of the above is generally correct.

C) low, positive or slightly negative

How many electrons in an atom can have the quantum numbers n = 3, l = 2? A. 2 B. 5 C. 10 D. 18 E. 6

C. 10

Which of the following is an incorrect designation for an atomic orbital? A. 1s B. 3d C. 1p D. 4f E. 6s

C. 1p

A given set of p orbitals consists of ______ orbitals. A. 2 B. 4 C. 3 D. 5 E. 1

C. 3

In the Lewis structure for ICl2-, how many lone pairs of electrons are around the central iodine atom? A. 2 B. 0 C. 3 D. 1 E. 4

C. 3

A given set of p orbitals consists of ______ orbitals. A. 1 B. 2 C. 3 D. 4 E. 5

C. 3 - Study Orbitals

How many d orbitals have n = 4? A. 7 B. 2 C. 5 D. 18 E. 10

C. 5

What is the correct symbol for silver? A. S B. Si C. Ag D. Sr E. Au

C. Ag

Which of the following is a reasonable criticism of the Bohr model of the atom? A. It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. B. It does not adequately predict the line spectrum of hydrogen. C. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. D. It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen. E. It shows the electrons to exist outside of the nucleus.

C. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.

Which of the following statements BEST describes the Heisenberg uncertainty principle? A. The exact position of an electron is always uncertain. B. The velocity of a particle can only be estimated. C. It is impossible to accurately know both the exact location and momentum of a particle. D. The location and momentum of a macroscopic object are not known with certainty. E. The location and momentum of a particle can be determined accurately, but not the identity of the particle.

C. It is impossible to accurately know both the exact location and momentum of a particle.

Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? A. ZnO2 and ZnCl2 B. H2O and HCl C. NO and NO2 D. CH4 and CO2 E. NH4 and NH4Cl

C. NO and NO2

Of the following elements, which needs three electrons to complete its valence shell? A. Cl B. Si C. P D. Ca E. Ba

C. P

Order the elements S, Cl, and F in terms of increasing ionization energy. A. Cl, F, S B. F, Cl, S C. S, Cl, F D. F, S, Cl E. S, F, Cl

C. S, Cl, F

Which of the following statements is true? A. All of the statements (A-C) are false. B. Ions are formed by adding or removing protons or electrons. C. Scientists believe that solids are mostly open space. D. At least two of the above statements (A-C) are true. E. Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases.

C. Scientists believe that solids are mostly open space.

Consider the following representation of a 2p-orbital: ８ - Not an Eight - more like a Infinity Symbol Standing Up. See Picture: Which of the following statements best describes the movement of electrons in a p-orbital? A. The electrons move along the outer surface of the p-orbital, similar to a "figure 8" type of movement. B. The electrons are concentrated at the center (node) of the two lobes. C. The electron movement cannot be exactly determined. D. The electrons are only moving in one lobe at any given time. E. The electrons move within the two lobes of the p-orbital, but never beyond the outside surface of the orbital.

C. The electron movement cannot be exactly determined.

Which of the following is incorrect? A. Diffraction produces both constructive and destructive interference. B. Niels Bohr developed a quantum model for the hydrogen atom. C. The emission spectrum of hydrogen contains a continuum of colors. D. All matter displays both particle and wavelike characteristics. E. The lowest possible energy state of a molecule or atom is called its ground state.

C. The emission spectrum of hydrogen contains a continuum of colors.

Which of the following is NOT determined by the principal quantum number, n, of the electron in a hydrogen atom? A. The energy of the electron. B. the minimum wavelength of the light needed to remove the electron from the atom. C. The size of the corresponding atomic orbital(s). D. The shape of the corresponding atomic orbital(s). E. All of the above are determined by n.

C. The size of the corresponding atomic orbital(s).

A pure substance composed of two or more different elements is a(n) ________. A. ion B. heterogeneous mixture C. chemical compound D. solid E. solution

C. chemical compound

Which of the following statements is false? A. In the usual order of filling, the 6s orbital is filled before the 4f orbital. B. The spin quantum number of an electron must be either + or -. C. The electron density at a point is proportional to ψ2 at that point. D. A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a 1s orbital. E. An orbital can accommodate at most two electrons.

D. A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a 1s orbital.

Hydrogen and lithium react very differently, although they are both members of Group 1. What is the primary reason for this difference? A. Electron affinity increases going down a group. B. The metallic character increases going down a group. C. The ionization energy increases going down a group. D. There is a very large difference in the atomic radii of H and Li. E. Electronegativity increases going down a group.

D. There is a very large difference in the atomic radii of H and Li.

In the Lewis structure for ICl2-, how many lone pairs of electrons are around the central iodine atom? A. 0 B. 1 C. 4 D. 3 E. 2

D. 3

Which of the following statements are false? I. It takes less energy to add an electron to nitrogen than to carbon because nitrogen will be closer to achieving a noble gas configuration. II. It takes more energy to add an electron to fluorine than to oxygen because the radius of fluorine is smaller and more repulsion would occur in the p-orbitals. III. It takes more energy to add an electron to nitrogen than to carbon because of the extra repulsions that would occur in the 2p orbitals. IV. Less energy is released in adding an electron to iodine than to chlorine because the radius of iodine is larger and the electron is added at a distance further from the nucleus. A. II, III B. I, II, IV C. III only D. I, II E. All of the above are false statements.

D. I, II Both of below are false. I. It takes less energy to add an electron to nitrogen than to carbon because nitrogen will be closer to achieving a noble gas configuration. II. It takes more energy to add an electron to fluorine than to oxygen because the radius of fluorine is smaller and more repulsion would occur in the p-orbitals.

The four lines observed in the visible emission spectrum of hydrogen tell us that: A. The hydrogen molecules they came from have the formula H4. B. We could observe more lines if we had a stronger prism. C. There are four electrons in an excited hydrogen atom. D. Only certain energies are allowed for the electron in a hydrogen atom. E. The spectrum is continuous.

D. Only certain energies are allowed for the electron in a hydrogen atom.

Which of the following pairs can be used to illustrate the law of multiple proportions? A. H2O and C12H22O11 B. CO and CaCO3 C. H2SO4 and H2S D. SO and SO2 E. KCl and KClO2

D. SO and SO2

Consider the ionization energy (IE) of the magnesium atom. Which of the following is not true? A. The IE of Mg is lower than that of Mg+. B. The IE of Mg is higher than that of calcium. C. The IE of Mg is lower than that of beryllium. D. The IE of Mg is lower than that of sodium. E. The IE of Mg is lower than that of neon.

D. The IE of Mg is lower than that of sodium.

Which of the following statements is true? A. The atomic radius of Li is larger than that of Cs. B. The ionization energy of S2- is greater than that of Cl-. C. The first ionization potential of H is greater than that of He. D. The ionic radius of Fe+ is larger than that of Fe3+. E. All are false.

D. The ionic radius of Fe+ is larger than that of Fe3+.

Which one of the following statements about atomic structure is false? A. An atom is mostly empty space. B. Almost all of the mass of the atom is concentrated in the nucleus. C. The protons and neutrons in the nucleus are very tightly packed. D. The number of protons and neutrons is always the same in the neutral atom. E. All of the above statements (A-D) are true.

D. The number of protons and neutrons is always the same in the neutral atom. (Think: Isotopes)

Which one of the following types of radiation has the shortest wavelength, the greatest energy, and the highest frequency? A. Infrared radiation. B. Visible red light. C. Visible blue light. D. Ultraviolet radiation. E. None, because short wavelength is associated with low energy and low frequency, not high energy and high frequency.

D. Ultraviolet radiation.

From the following list of observations, choose the one that most clearly supports the following conclusion: a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Electrons have wave properties.: A. observation a B. observation b C. observation c D. observation d E. observation e

D. observation d

An atom of fluorine contains nine electrons. How many of these electrons are in s orbitals? A. 8 B. 6 C. 2 D. 4 E. none

D.) 4

How many electrons can be contained in all of the orbitals with n = 4? A. 2 B. 8 C. 10 D. 18 E. 32

E. 32

How many electrons can be contained in all of the orbitals with n = 4? A. 18 B. 2 C. 8 D. 10 E. 32

E. 32 Shell = maximum electron capacity s = 2(1)^2 = 2 p = 2(2)^2 = 8 d = 2(3)^2 = 18 f = 2(4)^2 = 32 g = 2(5)^2 = 50

Alpha particles beamed at thin metal foil may: A. pass directly through without changing direction B. be slightly diverted by attraction to electrons C. be reflected by direct contact with nuclei D. A and C E. A, B, and C

E. A, B, and C A. pass directly through without changing direction B. be slightly diverted by attraction to electrons C. be reflected by direct contact with nuclei

Which of the following electron configurations is correct? A.Ga: [Kr]4s23d104p1 B. Br: [Kr]4s23d104p7 C. Mo: [Kr]5s24d5 D. Ca: [Ar]4s13d10 E. Bi: [Xe]6s24f145d106p3

E. Bi: [Xe]6s2 4f1 45d10 6p3

A hypothesis: A. Mathematical formula that models a pattern of behavior. B. Concise statement of a behavior that is always the same under the same conditions. C. Set of experiments designed to test a theory. D. Well-tested, unifying principle that explains a body of facts. E. Tentative explanation or prediction based upon experimental observations.

E. Tentative explanation or prediction based upon experimental observations.

Which of the following combinations of quantum numbers is not allowed? A. n = 3, l = 0, ml = 0, ms = - 1/2 B. n = 2, l = 1, ml = -1, ms = 1/2 C. n = 4, l = 3, ml = -2, ms = - 1/2 D. n = 4, l = 2, ml = 0, ms = 1/2 E. n = 1, l = 1, ml = 0, ms = 1/2

E. n = 1, l = 1, ml = 0, ms = 1/2

The first people to attempt to explain why chemical changes occur were: A. physicians B. metallurgists C. alchemists D. physicists E. the Greeks

E. the Greeks

The shape of an atomic orbital is associated with ... ? A. the magnetic quantum number (ml). B. the spin quantum number (ms). C. the principal quantum number (n). D. the magnetic and spin quantum numbers, together. E. the angular momentum quantum number (l).

E. the angular momentum quantum number (l)

Which of the following have 10 electrons in the "d" orbitals? A. Mn B. Fe C. Cu D. Zn E. two of the above

E. two of the above Cu: [Ar] 4s"1" 3d10 - Remember Cu is strange. Zn: [Ar] 4s2 3d10

Which of the following are incorrectly paired? A. wavelength - λ B. frequency - ν C. speed of light - c D. hertz - s-1 E. x-rays - shortest wavelength

E. x-rays - shortest wavelength

Enter the symbol of the element in the set below that is a metal. For example, H is the symbol of hydrogen. selenium, potassium, iodine Fill In Box:

Fill In Box: K

The __________ electrons are in the outermost principal quantum level of an atom.

Fill in Box - Valence

Electromagnetic radiation can be viewed as a stream of "particles" called __________. Fill In the Blank

Photons

The __________ quantum number is related to the size and energy of the orbital. Fill In Box

Principle

Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom? a. Planck b. Bohr c. Rydberg d. Rutherford e. Thomson

d. Rutherford

Which of the following statments is FALSE? a. Within a particular orbital, there can be only two electrons and they must both have the same spin. b. Shielding occurs when inner-shell electrons shield outer-shell electrons from the full attractive force of the nucleus. c. In a system of many electrons, the principal energy levels are split into sublevels of different energy. d. As the number of shielding electrons increases, the effective nuclear charge decreases. e. none of these is FALSE

a. Within a particular orbital, there can be only two electrons and they must both have the same spin.

Which of the following atoms has two unpaired electrons? a. He b. B c. Ca d. Se e. Zn

d. Se

The interference pattern seen when light passes through narrow, closely spaced slits, is due to a. diffraction. b. reflection. c. refraction. d. dispersion. e. deflection.

a. diffraction.

Millikan's oil-drop experiment: a. established the charge on an electron. b. showed that all oil drops carried the same charge. c. provided support for the nuclear model of the atom. d. suggested that some oil drops carried fractional numbers of electrons. e. suggested the presence of a neutral particle in the atom.

a. established the charge on an electron.

A column of the periodic table is called a a. group. b. period. c. isotopic mixture. d. pillar. e. shell.

a. group.

Pick the member of each pair with the greater bond energy. i) C-F or C-Cl ii) C-C bond in C2H4 or bond in F2 iii) C-O or C=O a. i) C-F ii) C2H4 iii) C=O b. i) C-F ii) F2 iii) C=O c. i) C-F ii) F2 iii) C-O d. i) C-Cl ii) C2H4 iii) C=O e. i) C-Cl ii) F2 iii) C-O

a. i) C-F ii) C2H4 iii) C=O

What keeps the electrons from leaving an atom in the Rutherford model of the atom? a. strong electrostatic attraction to the nucleus b. strong attraction to other electrons c. the repulsive forces between electrons d. an outer coating on the atom e. the orbits of the electrons are circular

a. strong electrostatic attraction to the nucleus

Select the correct formula for a compound formed from calcium and chlorine. a. CaCl b. CaCl2 c. Ca2Cl d. Ca2Cl2 e. CaCl3

b. CaCl2

Give the charge and full ground-state electron configuration of the monatomic ion most likely to be formed by the element: [Cl] a. Cl-: 1s22s22p63s23p5 b. Cl-: 1s22s22p63s23p6 c. Cl-: 1s22s22p63s23p4 d. Cl-: 1s22s22p63s23p64s e.none of these

b. Cl-: 1s22s22p63s23p6

Wherever it is found, water always contains oxygen and hydrogen in the mass ratio of 8 to 1. Taken by itself, this fact demonstrates what natural law? a. Conservation of Mass b. Definite Composition c. Multiple proportions d. The Atomic Theory e. Periodicity

b. Definite Composition

Which one of the following equations correctly represents the process involved in the electron affinity of X? a. X(g) → X+(g) + e¯ b. X+(g) → X+(aq) c. X+(g) + e¯ → X(g) d. X(g) + e¯ → X¯(g) e. X+(g) + Y¯(g) → XY(s)

d. X(g) + e¯ → X¯(g)

Which statement is true concerning atomic spectra? a. An emission spectrum (bright lines) is produced when atoms are excited to higher energy levels by simultaneously emitting photons. b. During the production of emission spectra, electrons move from higher to lower energy levels. c. Absorption spectra are seen as bright colored lines against a dark background. d. The emission spectrum of hydrogen consists of four lines but other elements have more lines. e. Each line in the emission spectrum of hydrogen represents one of the allowed energy levels in the hydrogen atom.

b. During the production of emission spectra, electrons move from higher to lower energy levels.

Pick the ion in each set with the smallest radius. i) O2-, F-, N3- ii) Na+, Mg2+, F- iii)Cr2+, Cr3+ a. F-, Na+, Cr2+ b. F-, Mg2+, Cr3+ c. N3-, Mg2+, Cr3+ d. O2-, Na+, Cr2+ e. N3-, F-, Cr2+

b. F-, Mg2+, Cr3+

Which is the most polar bond? a. I-Br b. K-Cl c. S-O d. O-Cl e. F-F

b. K-Cl Calculate the difference in electronegativity between two atoms. highest difference wins. obviously it's not E, since the difference is zero.

Energy states of atoms containing more than one electron are influenced by nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects? a. Larger nuclear charge lowers energy, more electrons in an orbital lowers energy. b. Larger nuclear charge lowers energy, more electrons in an orbital increases energy. c. Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy. d. Smaller nuclear charge lowers energy, more electrons in an orbital increases energy. e. None of these statements is generally correct.

b. Larger nuclear charge lowers energy, more electrons in an orbital increases energy.

Identify the mass law that each observation demonstrates. A flashbulb contains magnesium and oxygen before use and magnesium oxide afterward, but its mass does not change. a. Law of Definite Composition b. Law of Conservation of Mass c. Law of Multiple Proportions d. none of the above e. Law of Conservation of Mass and Law of Definite Composition

b. Law of Conservation of Mass

Which mass law(s) is/are demonstrated by the observation that a sample of potassium chloride from Chile contains the same percent by mass of potassium as one from Poland? a. Law of Conservation of Mass b. Law of Definite Composition c. Law of Multiple Proportions d. Law of Conservation of Mass & Definite Composition e. Law of Conservation of Mass & Multiple Proportions

b. Law of Definite Composition

Which ion or atom has the largest radius? a. Mg b. Na c. Na+ d. Mg2+ e. Al

b. Na

Which of the following ions and atoms has the largest radius? a. Mg b. Na c. Na+ d. Mg2+ e. Al

b. Na

Which of the following bonds has the greatest bond energy?

b. P-F

Which inventor/discovery is mismatched in the following list? a. Lavoisier: Law of Conservation of Mass b. Proust: mass of an electron c. Dalton : Atomic Theory of Matter d. Mendeleev: Periodic Table e. Arrhenius: acids produce H+ in water

b. Proust: mass of an electron

Which of the following experiments disproved Thompson's "raisin pudding" model of the atom? a. Millikan's oil drop experiment b. Rutherford's gold-foil experiment c. Michael Faraday's experiments with electric currents in air d. William Crookes cathode ray tube experiment e. Boyle's gas experiments

b. Rutherford's gold-foil experiment

What is the name of HClO3? a. hydrochloric acid b. chloric acid c. chlorous acid d. perchloric acid e. hypochlorous acid

b. chloric acid

According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 1 to n = 2 is ____ the energy necessary to excite an electron from n = 2 to n = 3. a. less than b. greater than c. equal to d. either equal to or greater than e. either less than or equal to

b. greater than

A row of the periodic table is called a: a. group. b. period. c. isotopic mixture. d. family. e. subshell.

b. period.

In an experiment searching for the photoelectric effect, an incident beam of green light produced no ejected electrons from a metal. In order to eject electrons, the experimenter should: a. increase the brightness of the light. b. try blue light. c. try yellow light. d. give up on that particular metal. e. decrease the brightness of the light.

b. try blue light.

Give the ground-state electron configuration, symbol, and group number from each partial (valence-level) orbital diagram. See Picture a. [Xe] 5s24d3; Ta; 5B (5) b. [Kr] 5s24d3; Nb; 5B (5) c. [Ar] 5s24d3; V; 5B (5) d. [Kr] 5s24d3; Tc; 7B (7) e. none of these

b.[Kr] 5s24d3; Nb; 5B (5)

What is the name of the element with the symbol B? a. barium b. beryllium c. bismuth d. boron e. bromine

d. boron

What is the name of BBr3? a. boron bromide b. boric bromide c. boron tribromide d. tribromoboride e. bromine triboride

d. tribromoboride

Which statement is NOT true concerning atomic spectra? a. An absorption spectrum is produced when atoms absorb certain wavelengths of incoming light. b. Electrons move from lower to higher energy levels when an absorption is produced. c. Absorption spectra and emission spectra of the same atom have the same appearance but the line frequencies are different. d. Absorption spectra are seen as dark lines against a bright background. e. Bohr based his model of the hydrogen atom on the emission spectra of hydrogen.

c. Absorption spectra and emission spectra of the same atom have the same appearance but the line frequencies are different.

Which of the following atoms has the most negative electron affinity? a. Se b. Al c. Cl d. Li e. More information is needed.

c. Cl

Which of the following elements has the most exothermic electron affinity? a. S b. As c. Cl d. Mg e. Ga

c. Cl

Which of the following elements, when combined with fluorine, would produce the most ionic bond? a. Ge b. Ru c. K d. N e. Mg

c. K

What is the identity of element Q if the ion Q2+ contains 10 electrons? a. O b. Ne c. Mg d. He e. Cr

c. Mg

Which of the following atoms is a non-metal? a. Fr b. Ge c. N d. Hg e. None of these are non-metals

c. N

Give the charge and full ground-state electron configuration of the monatomic ion most likely to be formed by the element. N a. N3-: 1s2 2s2 2p3 b. N4-: 1s2 2s1 c. N3-: 1s2 2s2 2p6 d. N4-: 1s2 2s2 2p6 3s1 e. none of these

c. N3-: 1s2 2s2 2p6

According to the law of multiple proportions: a. If the same two elements form two different compounds, they do so in the same ratio. b. The ratio of the masses of the elements in a compound is always the same. c. None of these. d. It is not possible for the same two elements to form more than one compound. e. The total mass after a chemical change is the same as before the change

c. None of these.

Which of the following bonds has the greatest bond energy? a. P-P b. P-F c. P-Cl d. P-Br e. P-I

c. P-Cl P-P -- 201 P-F -- 490 P-Cl -- 326 P-Br -- 264 P-I -- 184

Who is credited with measuring the mass/charge ratio of the electron? a. Dalton b. Gay-Lussac c. Thomson d. Millikan e. Rutherford

c. Thomson

The correct name of the compound N2O4 is a. nitric oxide. b. dinitrogen oxide. c. dinitrogen tetraoxide. d. nitrous oxide. e. nitrogen dioxide.

c. dinitrogen tetraoxide.

Rutherford's experiment with alpha particle scattering by gold foil established that: a. electrons have a negative charge. b. protons are 1840 times heavier than electrons. c. protons are not evenly distributed throughout an atom. d. atoms are made of protons, neutrons and electrons. e. the nucleus contains protons and neutrons.

c. protons are not evenly distributed throughout an atom. Bonus Info: - The atom is mostly empty space (because most α-particles were not deflected). - Most of the mass and all of the positive charge is concentrated in a tiny region at the centre. - This central nucleus only affected the α-particles when they came close to it.

The orientation in space of an atomic orbital is associated with ... ? a. the principal quantum number (n). b. the angular momentum quantum number (l). c. the magnetic quantum number (ml). d. the spin quantum number (ms). e. none of the above.

c. the magnetic quantum number (ml).

Rutherford bombarded gold foil with alpha (a) particles and found that a small percentage of the particles were deflected. Which of the following was not accounted for by the model he proposed for the structure of atoms? a. the small size of the nucleus b. the charge on the nucleus c. the total mass of the atom d. the existence of protons e. the presence of electrons outside the nucleus

c. the total mass of the atom

What is the atomic mass for the halogen that lies in period 5? a. 131.3 amu b. 127.6 amu c. approximately 210 d. 126.9 amu e. 53 amu

d. 126.9 amu

According to the Aufbau principle which sublevel is filled after the 5s sublevel? a. 5p b. 4f c. 3d d. 4d e. 5d

d. 4d

Which of the following subshell combinations are closest in energy in a typical polyelectron atom? a. 4s and 4p b. 5s and 3d c. 3d and 3s d. 4s and 3d e. 4p and 4d

d. 4s and 3d

Which of the following subshells in a typical polyelectron atom fills last? a. 1s b. 4d c. 4s d. 5p e. More information is needed.

d. 5p

Of the following elements, __________ has the most negative electron affinity. a. P b. Al c. Si d. Cl e. B

d. Cl

Which element among these has the most negative electron affinity (i.e., has most exothermic electron affinity). a. H b. Li c. C d. F e. Ne

d. F

Which mass law(s) is/are illustrated in the figure below? a. Law of conservation of mass b. Law of definite composition c. Law of multiple proportions d. Law of conservation of mass and law of definite composition e. Law of conservation of mass and law of multiple proportions f. Law of conservation of mass, law of definite composition and law of multiple proportions

d. Law of conservation of mass and law of definite composition

Which of the following sets has the compounds in order of decreasingly exothermic lattice energy? a. RbI, NaI, LiI, KI b. NaI, KI, RbI, LiI c. LiI, KI, RbI, NaI d. LiI, NaI, KI, RbI e. RbI, KI, NaI, LiI

d. LiI, NaI, KI, RbI

A compound of sulfur and oxygen is 50.0% sulfur, 50.0% oxygen by weight. Sulfur and oxygen form another compound, in accordance with the law of multiple proportions. Which of the following is a likely composition for the second compound? a. 85.0 mass % sulfur - 15.0 mass % oxygen. b. 65.0 mass % sulfur - 35.0 mass % oxygen. c. 55.0 mass % sulfur - 45.0 mass % oxygen. d. 45.0 mass % sulfur - 55.0 mass % oxygen. e. 40.0 mass % sulfur 60.0 mass % oxygen.

e. 40.0 mass % sulfur 60.0 mass % oxygen. Reason: 1 mole of SO2 consists of 1 mole of S (32.064g) and 2 moles of O (31.9988g), a 50/50 ratio. 1 mole of SO3 consists of 1 mole of S (32.064g) and 3 moles of O (47.9982g), a 2:3 (or 40:60) ratio.

How many unpaired electrons are there in a chromium atom (Z = 24) a. 0 b. 2 c. 3 d. 4 e. 6

e. 6

Which of these is NOT a characteristic of cathode rays? a. Follow straight line paths. b. Deflected by electrostatic charges c. Deflected by magnetic fields d. Consist of a type of subatomic particles that are present in all atoms. e. Always move toward the cathode (negative electrode).

e. Always move toward the cathode (negative electrode).

Which of the following has the largest radius? a. Na b. Cl- c. Rb+ d. Sr e. Cs

e. Cs

Which of the following atoms has four unpaired electrons? a. F b. Be c. C d. O e. Fe

e. Fe

Who is credited with discovering the atomic nucleus? a. Dalton b. Gay-Lussac c. Thomson d. Millikan e. Rutherford

e. Rutherford

What is the chemical symbol for the group 6A (16) element that lies in period 4? a. Cr b. Hf c. W d. Ti e. Se

e. Se

Which of the following elements is the LEAST electronegative? a. Si b. Se c. S d. Sc e. Sr

e. Sr It is the farthest to the left and down.

What type of spectrum, if any, would be produced if the light radiated by a heated atomic gas were to be dispersed through a prism? a. a continuous band of color b. a continuous band of color with some dark lines (missing wavelengths) c. only blue light d. only red light e. discrete lines of different colors

e. discrete lines of different colors

Which of these pairs is incorrect? a. aluminum - main group metal b. sulfur - main group nonmetal c. silicon - metalloid d. cobalt - transition metal e. gallium - main group nonmetal

e. gallium - main group nonmetal

Which of the following electron transitions will produce a photon of the longest wavelength in the Bohr hydrogen atom? a. n = 3 to n = 4 b. n = 4 to n = 1 c. n = 4 to n = 2 d. n = 1 to n = 5 e. n = 4 to n = 3

e. n = 4 to n = 3

Give the ground-state electron configuration, symbol, and group number from each partial (valence-level) orbital diagram. See Pic a. [He] 2s22p3; B; 3A (13) b. [Ne] 2s22p3; P; 5A (15) c. [He] 2s22p3; N; 7A (17) d. [Ar] 2s22p3; As; 5A (15) e. none of these

e. none of these

A zinc atom in its ground state has how many unpaired electrons? a. 1 b. 2 c. 12 d. 30 e. none of these

e. none of these None. Zinc fills up its 3d sublevel with 10 electrons, all pairs. So, there are no remaining unpaired electrons

Question 1 All the following are true EXCEPT a. the n = 3 shell has no f subshell b. there are three p orbitals in every shell of an atom except the n = 1 shell c. all s orbitals have spherical shapes d. each d subshell has five d orbitals e. the energies of subshell in the shells (energy levels) of a hydrogen atom vary as s < p < d, etc.

e. the energies of subshell in the shells (energy levels) of a hydrogen atom vary as s < p < d, etc.

When an atom is represented by the symbol (see below) Picture , the value of A is the: Image Shown was an element called X. Then to the left (on top) it has an "A" and then below the "A" is a "Z." a. number of neutrons in the atom. b. number of protons in the atom. c. atomic mass of the element. d. total number of electrons and neutrons in the atom. e. total number of protons and neutrons in the atom.

e. total number of protons and neutrons in the atom.

The most basic oxides are formed from elements found in the __________________ region of the periodic table.

lower left

Contact lenses can focus light due to the ___________ of the waves.

refraction

The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

upper right