Periodic Table Trends Quiz.2
This quiz is for all Chemistry students and lovers who are still struggling to comprehend the periodic table. Most of the times it is quite confusing and an application of the wrong periodic number makes a formula wrong. All the best!
- 1.
Ionization energy refers to
- A.
The energy needed to excite an electron
- B.
The energy needed to remove an electron
- C.
The energy needed to attract an electron
- D.
The energy needed to release a photon
Correct Answer
B. The energy needed to remove an electronExplanation
Ionization energy refers to the energy needed to remove an electron from an atom or ion in its ground state. This energy is required to overcome the attractive forces between the positively charged nucleus and the negatively charged electron. The higher the ionization energy, the more difficult it is to remove an electron, indicating a stronger hold of the electron by the nucleus.Rate this question:
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- 2.
Electronegativity refers to
- A.
The energy needed to excite an electron
- B.
The energy needed to remove an electron
- C.
The energy needed to attract an electron
- D.
The energy needed to release a photon
Correct Answer
C. The energy needed to attract an electronExplanation
Electronegativity refers to the energy needed to attract an electron. It is a measure of the ability of an atom to attract a shared pair of electrons towards itself in a chemical bond. Electronegativity increases across a period from left to right on the periodic table, and decreases down a group. This property is important in determining the type and strength of chemical bonds that can form between atoms.Rate this question:
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- 3.
The alkali metals family has _______ valence electrons.
- A.
1
- B.
2
- C.
6
- D.
7
- E.
8
Correct Answer
A. 1Explanation
The alkali metals family has 1 valence electron.Rate this question:
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- 4.
Magneiusm is in the __________ family.
- A.
Alkali metal
- B.
Alkaline earth metal
- C.
Transition metal
- D.
Chalcogen
- E.
Halogen
Correct Answer
B. Alkaline earth metalExplanation
Magnesium is in the alkaline earth metal family because it belongs to Group 2 of the periodic table. Alkaline earth metals are located in the second column of the periodic table and include elements such as beryllium, calcium, strontium, and barium. These elements have two valence electrons and are known for their high reactivity and ability to form 2+ cations. Magnesium shares these characteristics and therefore belongs to the alkaline earth metal family.Rate this question:
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- 5.
Which of the following elements is an alkali metal?
- A.
Hydrogen, H
- B.
Lithium, Li
- C.
Beryllium, Be
- D.
Vanadium, V
Correct Answer
B. Lithium, LiExplanation
Lithium is an alkali metal because it belongs to Group 1 of the periodic table, which consists of alkali metals. Alkali metals are highly reactive metals that are soft and have low melting points. They are known for their ability to readily lose their outermost electron to form a positive ion. Lithium exhibits these characteristics, making it an alkali metal.Rate this question:
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- 6.
Which element in period 5 has the largest atomic radii?
- A.
Rubidium, Rb
- B.
Xenon, Xe
- C.
Vanadium, V
- D.
Duborium, Db
Correct Answer
A. Rubidium, RbExplanation
Rubidium, Rb, has the largest atomic radii in period 5. Atomic radii generally decrease across a period from left to right due to an increase in the number of protons, which attracts the electrons more strongly and leads to a smaller atomic size. Rubidium is located on the far left side of period 5 and has the least number of protons, resulting in a larger atomic size compared to the other elements listed.Rate this question:
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- 7.
Which element in group 16 has the largest atomic radius?
- A.
Oxygen, O
- B.
Sulfur, S
- C.
Selenium, Se
- D.
Tellurium, Te
- E.
Polonium, Po
- F.
Ununhexium, Uuh
Correct Answer
F. Ununhexium, UuhExplanation
Ununhexium, also known as Uuh, has the largest atomic radius among the elements in group 16. This is because atomic radius generally increases as you move down a group in the periodic table. Since Ununhexium is located at the bottom of group 16, it has more electron shells compared to the other elements in the group, resulting in a larger atomic radius.Rate this question:
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- 8.
Which family consists primarily of large, radioactive, man-made elements?
- A.
Alkali metals
- B.
Transition metals
- C.
Lanthanides
- D.
Actinides
Correct Answer
D. ActinidesExplanation
The actinides family consists primarily of large, radioactive, man-made elements. These elements are located in the bottom row of the periodic table and are characterized by their high atomic numbers and unstable nuclei. They are all radioactive, meaning they undergo radioactive decay and emit radiation. Some examples of actinides include uranium, plutonium, and americium.Rate this question:
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- 9.
Which family is the least reactive?
- A.
Alkali metals
- B.
Chalcogens
- C.
Transition metalsals
- D.
Noble gases
Correct Answer
D. Noble gasesExplanation
Noble gases are the least reactive family because they have a full outer electron shell, making them stable and less likely to form chemical bonds with other elements. This stability is due to their complete valence electron configuration, which eliminates the need for them to gain or lose electrons to achieve a stable state. As a result, noble gases have very low reactivity and rarely participate in chemical reactions.Rate this question:
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- 10.
How many valence electrons does Helium (He) have?
- A.
1
- B.
2
- C.
7
- D.
8
Correct Answer
B. 2Explanation
Helium (He) has 2 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom, and they determine the atom's chemical properties and ability to form bonds with other atoms. Helium is in the second period of the periodic table, and it has a full 1s energy level with 2 electrons. Therefore, it has 2 valence electrons.Rate this question:
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- 11.
Why are halogens so highly reactive?
- A.
They have 1 valence electron and want to get rid of it
- B.
They have 1 valence electrons and want 7 more electrons
- C.
They have 7 valence electrons and want 1 more electron
- D.
They have 7 valence electrons and want to get rid of all 7 electrons
Correct Answer
C. They have 7 valence electrons and want 1 more electronExplanation
Halogens are highly reactive because they have 7 valence electrons and want to gain 1 more electron to achieve a stable octet configuration. This desire to gain one electron makes them highly reactive and prone to forming compounds with other elements.Rate this question:
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- 12.
What is the same within a period?
- A.
The number of valence electrons
- B.
The number of orbits/shells
- C.
The reactivity characteristics
- D.
The physical properties (color, melting point, boiling point)
Correct Answer
B. The number of orbits/shellsExplanation
Within a period, the number of orbits/shells remains the same. A period in the periodic table represents a specific energy level or shell in an atom. As you move across a period from left to right, the number of electrons in the outermost shell increases by one, but the number of shells remains constant. Therefore, the number of orbits/shells is the same within a period.Rate this question:
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- 13.
The most electronegative element on the periodic table is
- A.
Lithium, Li
- B.
Francium, Fr
- C.
Astatine, At
- D.
Fluorine, F
Correct Answer
D. Fluorine, FExplanation
Fluorine is the most electronegative element on the periodic table because it has the highest electronegativity value. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Fluorine has a strong attraction for electrons due to its small atomic size and high effective nuclear charge. This makes it highly reactive and capable of forming strong bonds with other elements. In comparison, Lithium, Francium, and Astatine have lower electronegativity values and are less capable of attracting electrons.Rate this question:
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- 14.
Iron, Fe is smaller than Hassium (Hs), primarily because
- A.
Iron has fewer neutrons
- B.
Iron has a smaller mass
- C.
Iron has a smaller atomic number
- D.
Iron has fewer orbits
Correct Answer
D. Iron has fewer orbitsExplanation
Iron, Fe, is smaller than Hassium, Hs, primarily because it has fewer orbits. The size of an atom is determined by the number of electrons and the energy levels or orbits they occupy. Iron has fewer orbits compared to Hassium, which means that the electrons in iron are closer to the nucleus and experience a stronger attractive force. This leads to a smaller atomic size for iron compared to Hassium.Rate this question:
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- 15.
The element with the lowest ionization energy periodic table is
- A.
Lithium, Li
- B.
Francium, Fr
- C.
Astatine, At
- D.
Fluorine, F
Correct Answer
B. Francium, FrExplanation
Francium, Fr, has the lowest ionization energy on the periodic table. Ionization energy is the energy required to remove an electron from an atom. Francium is located in the alkali metal group, which is known for having low ionization energies due to their large atomic size and low effective nuclear charge. As a result, francium has the lowest ionization energy among the given elements, making it the correct answer.Rate this question:
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- 16.
Electronegativity __________ as you go down a column because the electrons are ________ to/from the nucleus.
- A.
Increases, closer
- B.
Decreases, closer
- C.
Increases, farther
- D.
Decreases, farther
Correct Answer
D. Decreases, fartherExplanation
As you go down a column, electronegativity decreases because the electrons are farther from the nucleus. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. As you move down a column, the number of energy levels or shells increases, resulting in a greater distance between the outermost electrons and the nucleus. This increased distance weakens the attractive force between the nucleus and the electrons, leading to a decrease in electronegativity.Rate this question:
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- 17.
The elements Selenium (Se), Bromine (Br), and Nickel (Ni) are all in
- A.
Period 6
- B.
Group 6
- C.
Group 4
- D.
Period 4
Correct Answer
D. Period 4Explanation
The elements Selenium (Se), Bromine (Br), and Nickel (Ni) are all in period 4. Periods in the periodic table represent the number of electron shells or energy levels that an element's atoms have. Since all three elements are in the same period, it means that they have the same number of electron shells.Rate this question:
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- 18.
Atomic radius __________ as you go across a period because ________
- A.
Increases, there are more orbits
- B.
Increases, the nucleus pulls less on the electrons
- C.
Decreases, there are less orbits
- D.
Decreases, the nucleus pulls more on the electrons
Correct Answer
D. Decreases, the nucleus pulls more on the electronsExplanation
As you go across a period, the atomic radius decreases because the nucleus pulls more on the electrons. The atomic radius is the distance from the nucleus to the outermost electron shell. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger positive charge. This increased positive charge attracts the negatively charged electrons more strongly, pulling them closer to the nucleus. As a result, the atomic radius decreases.Rate this question:
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- 19.
Transition metals have _________ valence electrons.
- A.
Variable
- B.
2
- C.
6
- D.
8
Correct Answer
A. VariableExplanation
Transition metals typically have variable valence electrons. The number of valence electrons in transition metals can vary depending on the specific element and its oxidation state. Unlike alkali metals and alkaline earth metals, which have fixed valence electron configurations, transition metals can exhibit different oxidation states, leading to a variable number of valence electrons.Rate this question:
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- 20.
_______ is an example of a chalcogen
- A.
Lithium, Li
- B.
Barium, Ba
- C.
Selenium, Se
- D.
Neon, Ne
Correct Answer
C. Selenium, SeExplanation
Selenium is an example of a chalcogen. Chalcogens are a group of elements in the periodic table that includes oxygen, sulfur, selenium, tellurium, and polonium. They are known for their chemical properties, including their ability to form compounds with other elements. Selenium, with the symbol Se, is a nonmetallic element that belongs to this group. It is commonly used in various industrial applications, such as in the production of glass and electronics. Therefore, out of the given options, selenium is the correct answer as it is an example of a chalcogen.Rate this question:
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Feb 01, 2024Quiz Edited by
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Apr 11, 2011Quiz Created by
Lmmurp2
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