Chem B Unit 1 Practice Test
-
Write the full electron configuration for the following element. Aluminum Your answer should be in this format: 1s2 2s2 2p6 ... (there is a space between each orbital)
-
1s2 2s2 2p6 3s2 3p1
-
About This Quiz
This practice test includes topics that may appear on the Unit 1 test. This practice quiz is not intended to be the only study material you should use to study for the test.
Questions and Answers
- 2.
Write the full electron configuration for the following element. Sulfur Your answer should be in this format: 1s2 2s2 2p6 ... (there is a space between each orbital)
Explanation
The electron configuration of sulfur is 1s2 2s2 2p6 3s2 3p4. This means that sulfur has two electrons in the 1s orbital, two electrons in the 2s orbital, six electrons in the 2p orbital, two electrons in the 3s orbital, and four electrons in the 3p orbital.Rate this question:
- 3.
What element has the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Explanation
The given electron configuration corresponds to the element bromine. Bromine has an atomic number of 35, meaning it has 35 electrons. The electron configuration shows that bromine has 2 electrons in the 1s orbital, 2 electrons in the 2s orbital, 6 electrons in the 2p orbital, 2 electrons in the 3s orbital, 6 electrons in the 3p orbital, 2 electrons in the 4s orbital, 10 electrons in the 3d orbital, and 5 electrons in the 4p orbital. Therefore, the element with this electron configuration is bromine.Rate this question:
- 4.
Write the abbreviated (noble gas) electron configuration for the following element. Iodine Your answer should be in this format: [Ne] 3s2 3p6 ... (there is a space between each orbital)
- 5.
1.Which of the following CORRECTLY describes the modern periodic table?
-
It has 18 groups and 8 periods
-
It has 18 groups and 10 periods
-
It has 18 groups and 7 periods
-
It has 8 groups and 7 periods
Correct Answer
A. It has 18 groups and 7 periodsExplanation
The modern periodic table consists of 18 groups and 7 periods. The groups represent the columns of elements with similar properties, while the periods represent the rows of elements with increasing atomic numbers. This arrangement allows for the elements to be organized based on their chemical and physical properties, making it easier to study and understand their behavior.Rate this question:
-
- 6.
4.Which of the following groups in the periodic table contains a metalloid?
-
Group 2
-
Group 8
-
Group 14
-
Group 18
Correct Answer
A. Group 14Explanation
Group 14 in the periodic table contains a metalloid. Metalloids are elements that have properties of both metals and nonmetals. In Group 14, the element carbon is a nonmetal, while the elements silicon and germanium are metalloids. Therefore, Group 14 is the correct answer as it contains a metalloid.Rate this question:
-
- 7.
5.Which of the following elements will chlorine resemble closely in chemical properties?
-
Na
-
Br
-
Fe
-
O
Correct Answer
A. BrExplanation
Chlorine will closely resemble bromine (Br) in chemical properties because they both belong to the same group (Group 17 or Group VIIA) in the periodic table, known as the halogens. Halogens have similar chemical properties due to their similar electronic configurations and tendency to gain one electron to achieve a stable octet. Chlorine and bromine both have similar reactivity, electronegativity, and ability to form compounds with other elements.Rate this question:
-
- 8.
Write the symbol of the elements that fits the given description. the alkali metal with the highest atomic mass
Correct Answer
FrExplanation
Fr is the symbol for francium, which is an alkali metal. Francium has the highest atomic mass among all the alkali metals.Rate this question:
- 9.
Write the symbol of the elements that fits the given description. the noble gas with the lowest atomic mass
Correct Answer
HeExplanation
Helium (He) is the noble gas with the lowest atomic mass. It has an atomic number of 2 and an atomic mass of 4.0026 atomic mass units. Helium is the second lightest element in the periodic table, after hydrogen. It is a colorless, odorless, and non-reactive gas that is commonly used in balloons and as a cooling agent in various industries.Rate this question:
- 10.
EM Waves travel at the constant speed of?
-
Light
-
Sound
-
Energy
-
Unknown
Correct Answer
A. LightExplanation
EM waves, or electromagnetic waves, travel at the constant speed of light. This is a fundamental property of light, as it is an electromagnetic wave itself. The speed of light in a vacuum is approximately 299,792,458 meters per second, and this speed is constant regardless of the frequency or wavelength of the light. This constant speed of light is a cornerstone of Einstein's theory of relativity and has been confirmed by numerous experiments and observations. Therefore, the correct answer is light.Rate this question:
-
- 11.
The distance between crests is know as?
-
Crest Distance
-
Unknown Distance
-
Wavelength
-
Variable Distance
Correct Answer
A. WavelengthExplanation
The distance between crests is known as the wavelength. This term is commonly used in physics and refers to the length of one complete wave cycle. It is measured from one crest to the next crest, or from one trough to the next trough, depending on the type of wave. Wavelength is an important concept in understanding wave behavior and is often used to describe various types of waves, such as electromagnetic waves and sound waves.Rate this question:
-
- 12.
Wavelengths are measured in?
-
Meters & Nanometers
-
Feet & Inches
-
Inches & Centimeters
-
Inches to CM Cal
Correct Answer
A. Meters & NanometersExplanation
Wavelengths are measured in meters and nanometers. Meters are commonly used to measure longer wavelengths, such as those in the visible light spectrum, while nanometers are used to measure shorter wavelengths, such as those in the ultraviolet or infrared spectrum. This measurement system allows for precise and accurate characterization of the size and frequency of waves in various scientific and technological applications.Rate this question:
-
- 13.
The amount of crests that pass a given point within one second is discribed as the?
-
Pass Point
-
Ultraviolet Pass Point
-
Crest Point Through
-
Frequency
Correct Answer
A. FrequencyExplanation
The correct answer is "Frequency." Frequency refers to the number of crests (or any other wave component) that pass a specific point within one second. It is a measure of how often a wave completes one cycle. In the context of the given question, frequency is the appropriate term to describe the amount of crests passing a given point in one second.Rate this question:
-
- 14.
Radio waves have the lowest?
-
Facebook accounts
-
Wave Turn
-
Frequency
-
Point of Turn
Correct Answer
A. FrequencyExplanation
Radio waves have the lowest frequency among the given options. Frequency refers to the number of complete cycles of a wave that occur in a given amount of time. In the case of radio waves, they have a lower frequency compared to other types of waves such as visible light or microwaves. This low frequency allows radio waves to have a longer wavelength, which is why they are commonly used for long-distance communication.Rate this question:
-
- 15.
Red has the shortest wavelength
-
True
-
False
Correct Answer
A. FalseExplanation
The statement "Red has the shortest wavelength" is incorrect. In the visible light spectrum, red light has the longest wavelength, while violet light has the shortest wavelength. This is because wavelength and color are inversely related - shorter wavelengths correspond to higher frequency and bluer colors, while longer wavelengths correspond to lower frequency and redder colors.Rate this question:
-
- 16.
Violet has the longest wavelength
-
True
-
False
Correct Answer
A. FalseExplanation
The statement "Violet has the longest wavelength" is incorrect. In the visible light spectrum, violet light has the shortest wavelength, while red light has the longest wavelength.Rate this question:
-
- 17.
Which of the following options is true for the periodic table trend for ionization energy?
-
Ionization energy increases across a row and decreases down a group
-
Ionization energy increases across a row and increases down a group
-
Ionization energy decreases across a row and increases down a group
-
Ionization energy decreases across a row and decreases down a group
Correct Answer
A. Ionization energy increases across a row and decreases down a groupExplanation
The ionization energy trend in the periodic table is that it increases across a row and decreases down a group. This means that it takes more energy to remove an electron from an atom as you move across a row from left to right due to the increasing number of protons in the nucleus. On the other hand, it takes less energy to remove an electron as you move down a group due to the increasing distance between the nucleus and the outermost electrons.Rate this question:
-
- 18.
The energy required to remove an electron from an atom is known as:
-
Reactivity
-
Electron affinity
-
Electronegativity
-
Ionization energy
Correct Answer
A. Ionization energyExplanation
Ionization energy is the correct answer because it refers to the energy required to remove an electron from an atom. This process involves overcoming the attractive forces between the negatively charged electron and the positively charged nucleus. The higher the ionization energy, the more difficult it is to remove an electron, indicating a greater stability of the atom. Ionization energy is an important concept in understanding chemical reactions and the behavior of elements in the periodic table.Rate this question:
-
- 19.
The measure of the attraction that an atom has for electrons involved in chemical bonds is known as:
-
Electron affinity
-
Electronegativity
-
Ionization Energy
-
Reactivity
Correct Answer
A. ElectronegativityExplanation
Electronegativity refers to the measure of an atom's attraction towards electrons involved in chemical bonds. It indicates the ability of an atom to attract shared electrons towards itself. This property helps determine the polarity of a chemical bond and the distribution of electron density within a molecule. It is an essential concept in understanding chemical bonding and the reactivity of different elements.Rate this question:
-
- 20.
Which of the following element has the largest first ionization energy?
-
Oxygen
-
Fluorine
-
Carbon
-
Bromine
Correct Answer
A. FluorineExplanation
Fluorine has the largest first ionization energy among the given elements. Ionization energy is the energy required to remove an electron from an atom. Fluorine has the highest electronegativity value, indicating its strong attraction for electrons. This strong attraction makes it difficult to remove an electron from a fluorine atom, resulting in a high ionization energy. Oxygen has a slightly lower ionization energy than fluorine, while carbon and bromine have even lower ionization energies.Rate this question:
-
- 21.
Anions have a ______________ charge and are ______________ than the atoms from which they formed.
-
Positive/smaller
-
Positive/larger
-
Negative/smaller
-
Negative/larger
Correct Answer
A. Negative/largerExplanation
Anions have a negative charge because they have gained one or more electrons. When atoms gain electrons to become anions, they become larger in size because the additional electrons increase the electron-electron repulsion, causing the electron cloud to expand. Therefore, anions are negatively charged and larger than the atoms from which they formed.Rate this question:
-
- 22.
Which of the following element has the smallest first ionization energy?
-
Oxygen
-
Phosphor
-
Sodium
-
Sulfur
Correct Answer
A. SodiumExplanation
Sodium has the smallest first ionization energy compared to the other elements listed. First ionization energy is the energy required to remove the outermost electron from an atom. Sodium has a single electron in its outermost energy level, which is relatively far from the nucleus and experiences less attraction. This makes it easier to remove the electron, resulting in a lower ionization energy compared to the other elements listed.Rate this question:
-
- 23.
In the periodic table trend for atomic radius, the atomic radius decreases across a period and increases down a group.
-
True
-
False
Correct Answer
A. TrueExplanation
The statement is true because as you move across a period in the periodic table, the number of protons and electrons increases, resulting in a stronger attraction between the positively charged nucleus and the negatively charged electrons. This causes the electrons to be pulled closer to the nucleus, making the atomic radius smaller. On the other hand, as you move down a group, the number of energy levels or shells increases, leading to a larger atomic radius due to the increased distance between the nucleus and the outermost electrons.Rate this question:
-
- 24.
How many valence electrons do the Alkali Metals have?
Correct Answer
1Explanation
The alkali metals, which include elements like lithium, sodium, and potassium, all have one valence electron. Valence electrons are the electrons in the outermost energy level of an atom and are responsible for the chemical behavior of an element. In the case of alkali metals, they have one valence electron in their outermost energy level, making them highly reactive and likely to lose that electron to form a positive ion. Therefore, the correct answer is 1.Rate this question:
- 25.
How many valence electrons do the Alkaline Earth metals have?
Correct Answer
2Explanation
The Alkaline Earth metals have 2 valence electrons. This is because they belong to Group 2 of the periodic table, which means they have 2 electrons in their outermost energy level. Valence electrons are the electrons involved in chemical bonding, and having 2 valence electrons makes the Alkaline Earth metals chemically reactive.Rate this question:
- 26.
How many valence electrons do the elements in Group 13 have?
Correct Answer
3Explanation
The elements in Group 13 of the periodic table have 3 valence electrons. This is because Group 13 elements have three electrons in their outermost energy level, which is also known as the valence shell. Valence electrons are the electrons involved in chemical bonding and determine the reactivity of an element. Therefore, the elements in Group 13 have 3 valence electrons.Rate this question:
- 27.
How many valence electrons do the Halogens have?
Correct Answer
7Explanation
Halogens are a group of elements in the periodic table that include fluorine, chlorine, bromine, iodine, and astatine. They are located in Group 17, also known as Group VIIA. The number 7 represents the number of valence electrons that halogens have. Valence electrons are the outermost electrons in an atom and are involved in chemical bonding. Since halogens have 7 valence electrons, they are highly reactive and tend to gain one electron to achieve a stable electron configuration of 8 electrons in their outermost energy level.Rate this question:
- 28.
Which of the following elements has the smallest atomic radius?
-
Aluminum
-
Fluorine
-
Potassium
-
Sulfur
Correct Answer
A. FluorineExplanation
Fluorine has the smallest atomic radius among the given elements. Atomic radius refers to the size of an atom, which is determined by the distance between the nucleus and the outermost electron shell. Fluorine has a higher effective nuclear charge, meaning that the positive charge of the nucleus is stronger, pulling the electrons closer to the nucleus. This results in a smaller atomic radius compared to the other elements listed.Rate this question:
-
- 29.
The least electronegative elements are the:
-
Metalloids
-
Alkali metals
-
Alkaline Earth metals
-
Transition metals
-
Noble Gases
-
Halogens
Correct Answer
A. Noble GasesExplanation
Noble gases are the least electronegative elements because they have a full valence shell of electrons and are therefore stable and unreactive. Electronegativity is the tendency of an atom to attract electrons towards itself in a chemical bond, and noble gases do not readily attract or share electrons with other atoms due to their stable electron configuration. In contrast, metalloids, alkali metals, alkaline earth metals, transition metals, and halogens all have a higher electronegativity because they either have a tendency to gain or lose electrons to achieve a stable electron configuration.Rate this question:
-
Quiz Review Timeline (Updated): Mar 15, 2023 +
Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.
-
Current Version
-
Mar 15, 2023Quiz Edited by
ProProfs Editorial Team -
Mar 31, 2015Quiz Created by
AnnMarie Willette
Back to top