Chapter 3: Problem 103
Of the elements \(\mathrm{Li}, \mathrm{Be}, \mathrm{N}\), and \(\mathrm{F}\), which a. is an alkaline earth metal? b. has the largest atomic radius? c. has the highest ionization energy? \(\mathbf{d}\). is found in Group \(5 \mathrm{~A}(15) ?\)
Short Answer
Expert verified
a. Be, b. Li, c. F, d. N
Step by step solution
01
Identify Alkaline Earth Metal
Alkaline earth metals are elements in Group 2 of the periodic table. These elements are known to have two electrons in their outer shell.
02
Check Group 2 Elements
The elements provided are \(\text{Li}\), \(\text{Be}\), \(\text{N}\), and \(\text{F}\). From this list, \(\text{Be}\) (Beryllium) is the only element that is an alkaline earth metal.
03
Identify Largest Atomic Radius
Atomic radius generally increases down a group and decreases across a period. Therefore, the element with the fewest protons will generally have the largest atomic radius. Comparing \(\text{Li}\), \(\text{Be}\), \(\text{N}\), and \(\text{F}\), \(\text{Li}\) (Lithium) has the largest atomic radius.
04
Identify Highest Ionization Energy
Ionization energy increases across a period from left to right and decreases down a group. Between \(\text{Li}\), \(\text{Be}\), \(\text{N}\), and \(\text{F}\), \(\text{F}\) (Fluorine) has the highest ionization energy.
05
Identify Group 5A (15) Element
Group 5A (15) of the periodic table contains elements with five valence electrons. From the given elements, \(\text{N}\) (Nitrogen) fits this description.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
alkaline earth metals
Alkaline earth metals belong to Group 2 of the periodic table. They include elements like Beryllium (Be), Magnesium (Mg), Calcium (Ca), and others. These elements are known for having two electrons in their outermost shell, which gives them specific chemical properties. For example, these metals are typically shiny, reactive (though not as reactive as alkali metals from Group 1), and have higher melting points than Group 1 elements.
- Alkaline earth metals easily form compounds with other elements.
- They are usually found in the Earth's crust only in compound form because of their reactivity.
atomic radius
The atomic radius refers to the distance from the center of an atom's nucleus to the outermost electron shell. This is important because it influences an element's reactivity and bonding characteristics. Atomic radius generally increases as you move down a group and decreases as you move from left to right across a period.
- Down a group: Electrons are added to new shells, making the atom larger.
- Across a period: Additional protons pull the electron cloud closer to the nucleus, reducing the atomic size.
ionization energy
Ionization energy is the amount of energy required to remove an electron from a neutral atom in its gaseous phase. This property helps understand how strongly an atom holds onto its electrons. Ionization energy generally increases across a period from left to right and decreases down a group.
- Across a period: Atoms have more protons, increasing nuclear charge and holding electrons more tightly.
- Down a group: Electrons are farther from the nucleus and feel less pull, making them easier to remove.
group 5A elements
Group 5A elements, also known as Group 15 elements, contain five valence electrons. This group includes elements like Nitrogen (N), Phosphorus (P), Arsenic (As), and others. These elements have varied chemical properties, but typically, they can form three bonds with other elements due to their five valence electrons.
- These elements can show multiple oxidation states.
- They are important in both organic and inorganic chemistry.