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Chapter 4: Problem 9

Give the symbol of the element described by each of the following: a. Group \(4 \mathrm{~A}\) (14), Period 2 b. the noble gas in Period 1 c. the alkali metal in Period 3 d. Group \(2 \mathrm{~A}\) (2), Period 4 e. Group \(3 \mathrm{~A}\) (13), Period 3

Short Answer

Expert verified
a. C, b. He, c. Na, d. Ca, e. Al

Step by step solution

01

Identify element in Group 4A (14), Period 2

Find the element that is located in Group 4A (14) and Period 2 of the periodic table. Since Group 4A is the group that contains 4 valence electrons, and Period 2 indicates the second row, the element is Carbon (C).
02

Identify the noble gas in Period 1

Noble gases are located in Group 18 of the periodic table. For Period 1, the noble gas is Helium (He).
03

Identify the alkali metal in Period 3

Alkali metals belong to Group 1 of the periodic table. For Period 3, the alkali metal is Sodium (Na).
04

Identify element in Group 2A (2), Period 4

Group 2A elements are alkaline earth metals. In Period 4, the element belonging to Group 2A is Calcium (Ca).
05

Identify element in Group 3A (13), Period 3

Group 3A elements have 3 valence electrons. In Period 3, the element in Group 3A is Aluminum (Al).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

periodic table groups
The periodic table is arranged in rows called periods and columns called groups.
Groups are the vertical columns and are numbered from 1-18.
Each group has elements with similar chemical properties.
For example, all elements in Group 1 are called alkali metals, and they share properties like being highly reactive.
Another important group is Group 18, known as the noble gases, which are very stable and nonreactive.
valence electrons
Valence electrons are the outermost electrons of an atom and are involved in chemical bonding.
Elements in the same group typically have the same number of valence electrons.
For instance, elements in Group 1 have one valence electron, and elements in Group 17 have seven valence electrons.
Valence electrons play a crucial role in determining how an element will react chemically with others.
alkali metals
Alkali metals belong to Group 1 of the periodic table.
This group includes elements like Lithium (Li), Sodium (Na), and Potassium (K).
Alkali metals are characterized by having a single valence electron, which makes them highly reactive, especially with water.
These elements are soft, silvery metals that can be easily cut with a knife.
noble gases
Noble gases are in Group 18 of the periodic table.
Examples include Helium (He), Neon (Ne), and Argon (Ar).
These elements are known for their lack of reactivity due to having a complete set of valence electrons.
This makes them very stable and thus they rarely form compounds.
Noble gases are often used in lighting and inert environments due to their stability.
alkaline earth metals
Alkaline earth metals are found in Group 2 of the periodic table and include elements like Magnesium (Mg) and Calcium (Ca).
These elements have two valence electrons, which they readily lose to form +2 ions.
They are not as reactive as alkali metals but still react with water and oxygen.
Alkaline earth metals are harder and have higher melting points than alkali metals.

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Most popular questions from this chapter

Indicate if each of the following statements is true or false: \((4.3)\) a. The proton is a negatively charged particle. b. The neutron is 2000 times as heavy as a proton. c. The atomic mass unit is based on a carbon atom with 6 protons and 6 neutrons. d. The nucleus is the largest part of the atom. e. The electrons are located outside the nucleus.

Zinc consists of five naturally occurring isotopes: \({ }_{30}^{64} \mathrm{Zn}\), \(\frac{66}{30} \mathrm{Zn},{ }_{30}^{67} \mathrm{Zn},{ }_{30}^{68} \mathrm{Zn}\), and \({ }_{30}^{70} \mathrm{Zn}\). None of these isotopes has the atomic mass of \(65.41\) listed for zinc on the periodic table. Explain.

Identify the group or period number described by each of the following: a. contains \(\mathrm{Na}, \mathrm{K}\), and \(\mathrm{Rb}\) b. begins with \(\mathrm{Be}\) c. contains the noble gases d. contains \(\mathrm{B}, \mathrm{N}\), and \(\mathrm{F}\)

Strontium has four naturally occurring isotopes, with mass numbers \(84,86,87\), and 88 . a. Write the atomic symbol for each of these atoms. b. How are these isotopes alike? c. How are they different? d. Why is the atomic mass of strontium listed on the periodic table not a whole number? e. Which isotope is the most prevalent in a sample of strontium?

Silicon has three naturally occurring isotopes: \(\mathrm{Si}-28\) that has a percent abundance of \(92.23 \%\) and a mass of \(27.977 \mathrm{amu}, \mathrm{Si}-29\) that has a \(4.68 \%\) abundance and a mass of \(28.976 \mathrm{amu}\), and Si- 30 that has a \(3.09 \%\) abundance and a mass of \(29.974\) amu. Calculate the atomic mass for silicon using the weighted average mass method. \((4.5)\)
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