Questions and Answers
Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table?
The number of principle energy levels increases, and the number of valence electrons remains the same.
What is the total number of valence electrons in an atom of boron in the ground state?
3
What is the total number of valence electrons in an atom of xenon, Xe?
8
The elements calcium and strontium have similar chemical properties because they both have the same?
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On the Periodic Table of the Elements, all the elements within Group 16 have the same number of?
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An element with a partially filled d sublevel in the ground state is classified as?
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Which electron configuration represents a transition element?
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Which element in period 5 of the Periodic Table is a transition element?
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Which of the following atoms has the largest atomic radius?
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Which noble gas has the highest first ionization energy?
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Which sequence of elements is arranged in order of decreasing atomic radii?
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Which list of elements from group 2 on the Periodic Table is arranged in order of increasing atomic radius?
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As each successive element in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius?
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The strength of an atom's attraction for the electrons in a chemical bond is the atom's?
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Which properties are most common in nonmetals?
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Which Group 17 element has the least attraction for electrons?
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Which element in Group 16 has the greatest tendency to gain electrons?
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The Group 17 element with the highest electronegativity is?
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As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally?
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The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as?
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Which element is a member of the halogen family?
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Which of the following Group 2 elements has the lowest first ionization energy?
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As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to?
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Which sequence correctly places the elements in order of increasing ionization energy?
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Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having?
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Which of the elements has the least attraction for electrons in a chemical bond?
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The ability of carbon to attract electrons is?
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As the elements Li to F in period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare?
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Study Notes
Group Trends in the Periodic Table
- Group 2 elements show an increase in principal energy levels while maintaining the same number of valence electrons.
- All Group 16 elements possess the same number of valence electrons, influencing their chemical properties.
- Elements in Group 1, when analyzed top to bottom, exhibit decreasing ionization energy due to increasing atomic radius and shielding effect.
Valence Electrons and Ionization Energy
- Boron has 3 valence electrons in its ground state.
- Xenon, a noble gas, has a total of 8 valence electrons.
- The first ionization energy refers to the energy needed to remove the outermost electron from a gaseous atom in the ground state.
Atomic Radius Trends
- Atomic radius tends to decrease across a period and increases down a group.
- Example sequence of decreasing atomic radius: Al > Si > P.
- Group 2 elements arranged in increasing atomic radius: Be < Mg < Ca.
- Potassium (K) has the largest atomic radius among given atom options.
Electronegativity and Chemical Properties
- The strength of an atom's attraction for electrons in a bond is termed electronegativity.
- Nonmetals commonly exhibit high ionization energy and high electronegativity.
- Fluorine is the Group 17 element with the highest electronegativity, while iodine (I) has the least attraction for electrons.
Transition Metals and Electron Configuration
- Transition metals are characterized by partially filled d sublevels.
- Example of a transition element electron configuration is [Ar] 3d5 4s2.
- Silver (Ag) is a transition element located in period 5.
Special Cases in Groups
- Oxygen (O) in Group 16 has the greatest tendency to gain electrons.
- Barium (Ba) from Group 2 has the lowest first ionization energy.
- Nitrogen exhibits the least attraction for electrons in a chemical bond compared to other elements.
Comparison of Elements
- Relative electronegativity of elements increases while atomic radius decreases from lithium (Li) to fluorine (F) in period 2.
- Magnesium has a smaller atomic radius than sodium due to a larger nuclear charge.
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Description
Test your knowledge of periodic trends with these flashcards. Each card presents key concepts related to group elements, valence electrons, and the structure of the periodic table. Perfect for students studying chemistry and wanting to strengthen their understanding.
