Learning Objectives

• Atoms Of Elements That Are In The Same Group Have The Same Number Of Quizlet
• Atoms Of Elements That Are In The Same Group Have The Same Number Of What

For consecutive elements proceeding down any group, anions have larger principal quantum numbers and, thus, larger radii. Atoms and ions that have the same electron configuration are said to be isoelectronic. Examples of isoelectronic species are N 3–, O 2–, F –, Ne, Na +, Mg 2+, and Al 3+ (1s 2 2s 2 2p 6). In many cases, elements that belong to the same group (vertical column) on the periodic table form ions with the same charge because they have the same number of valence electrons. Thus, the periodic table becomes a tool for remembering the charges on many ions.

By the end of this section, you will be able to:

Elements located in the vertical column of the periodic table are of the same and have chemical properties. Two completely different compounds may contain identical elements. In a chemical formula, the number of atoms for each element is usually indicated by a. The order of elements in the modern periodic table is based on an element's atomic number. Elements within the same group in the periodic table have similar properties because they have the same.

• State the periodic law and explain the organization of elements in the periodic table
• Predict the general properties of elements based on their location within the periodic table
• Identify metals, nonmetals, and metalloids by their properties and/or location on the periodic table

As early chemists worked to purify ores and discovered more elements, they realized that various elements could be grouped together by their similar chemical behaviors. One such grouping includes lithium (Li), sodium (Na), and potassium (K): These elements all are shiny, conduct heat and electricity well, and have similar chemical properties. A second grouping includes calcium (Ca), strontium (Sr), and barium (Ba), which also are shiny, good conductors of heat and electricity, and have chemical properties in common. However, the specific properties of these two groupings are notably different from each other. For example: Li, Na, and K are much more reactive than are Ca, Sr, and Ba; Li, Na, and K form compounds with oxygen in a ratio of two of their atoms to one oxygen atom, whereas Ca, Sr, and Ba form compounds with one of their atoms to one oxygen atom. Fluorine (F), chlorine (Cl), bromine (Br), and iodine (I) also exhibit similar properties to each other, but these properties are drastically different from those of any of the elements above.

Dimitri Mendeleev in Russia (1869) and Lothar Meyer in Germany (1870) independently recognized that there was a periodic relationship among the properties of the elements known at that time. Both published tables with the elements arranged according to increasing atomic mass. But Mendeleev went one step further than Meyer: He used his table to predict the existence of elements that would have the properties similar to aluminum and silicon, but were yet unknown. The discoveries of gallium (1875) and germanium (1886) provided great support for Mendeleev’s work. Although Mendeleev and Meyer had a long dispute over priority, Mendeleev’s contributions to the development of the periodic table are now more widely recognized (Figure 1).

Figure 1. (a) Dimitri Mendeleev is widely credited with creating (b) the first periodic table of the elements. (credit a: modification of work by Serge Lachinov; credit b: modification of work by “Den fjättrade ankan”/Wikimedia Commons)

By the twentieth century, it became apparent that the periodic relationship involved atomic numbers rather than atomic masses. The modern statement of this relationship, the periodic law, is as follows: the properties of the elements are periodic functions of their atomic numbers. A modern periodic table arranges the elements in increasing order of their atomic numbers and groups atoms with similar properties in the same vertical column (Figure 2). Each box represents an element and contains its atomic number, symbol, average atomic mass, and (sometimes) name. The elements are arranged in seven horizontal rows, called periods or series, and 18 vertical columns, called groups. Groups are labeled at the top of each column. In the United States, the labels traditionally were numerals with capital letters. However, IUPAC recommends that the numbers 1 through 18 be used, and these labels are more common. For the table to fit on a single page, parts of two of the rows, a total of 14 columns, are usually written below the main body of the table.

Figure 2. Elements in the periodic table are organized according to their properties.

Many elements differ dramatically in their chemical and physical properties, but some elements are similar in their behaviors. For example, many elements appear shiny, are malleable (able to be deformed without breaking) and ductile (can be drawn into wires), and conduct heat and electricity well. Other elements are not shiny, malleable, or ductile, and are poor conductors of heat and electricity. We can sort the elements into large classes with common properties: metals (elements that are shiny, malleable, good conductors of heat and electricity—shaded yellow); nonmetals (elements that appear dull, poor conductors of heat and electricity—shaded green); and metalloids (elements that conduct heat and electricity moderately well, and possess some properties of metals and some properties of nonmetals—shaded purple).

The elements can also be classified into the main-group elements (or representative elements) in the columns labeled 1, 2, and 13–18; the transition metals in the columns labeled 3–12; and inner transition metals in the two rows at the bottom of the table (the top-row elements are called lanthanides and the bottom-row elements are actinides; Figure 3). The elements can be subdivided further by more specific properties, such as the composition of the compounds they form. For example, the elements in group 1 (the first column) form compounds that consist of one atom of the element and one atom of hydrogen. These elements (except hydrogen) are known as alkali metals, and they all have similar chemical properties. The elements in group 2 (the second column) form compounds consisting of one atom of the element and two atoms of hydrogen: These are called alkaline earth metals, with similar properties among members of that group. Other groups with specific names are the pnictogens (group 15), chalcogens (group 16), halogens (group 17), and the noble gases (group 18, also known as inert gases). The groups can also be referred to by the first element of the group: For example, the chalcogens can be called the oxygen group or oxygen family. Hydrogen is a unique, nonmetallic element with properties similar to both group 1A and group 7A elements. For that reason, hydrogen may be shown at the top of both groups, or by itself.

Figure 3. The periodic table organizes elements with similar properties into groups.

Example 1: Naming Groups of Elements

Atoms of each of the following elements are essential for life. Give the group name for the following elements:

1. chlorine
2. calcium
3. sodium
4. sulfur

Atoms Of Elements That Are In The Same Group Have The Same Number Of Quizlet

1. halogen
2. alkaline earth metal
3. alkali metal
4. chalcogen

Check Your Learning

Give the group name for each of the following elements:

1. krypton
2. selenium
3. barium
4. lithium

1. noble gas
2. chalcogen
3. alkaline earth metal
4. alkali metal

In studying the periodic table, you might have noticed something about the atomic masses of some of the elements. Element 43 (technetium), element 61 (promethium), and most of the elements with atomic number 84 (polonium) and higher have their atomic mass given in square brackets. This is done for elements that consist entirely of unstable, radioactive isotopes (you will learn more about radioactivity in the nuclear chemistry chapter). An average atomic weight cannot be determined for these elements because their radioisotopes may vary significantly in relative abundance, depending on the source, or may not even exist in nature. The number in square brackets is the atomic mass number (and approximate atomic mass) of the most stable isotope of that element.

Key Concepts and Summary

The discovery of the periodic recurrence of similar properties among the elements led to the formulation of the periodic table, in which the elements are arranged in order of increasing atomic number in rows known as periods and columns known as groups. Elements in the same group of the periodic table have similar chemical properties. Elements can be classified as metals, metalloids, and nonmetals, or as a main-group elements, transition metals, and inner transition metals. Groups are numbered 1–18 from left to right. The elements in group 1 are known as the alkali metals; those in group 2 are the alkaline earth metals; those in 15 are the pnictogens; those in 16 are the chalcogens; those in 17 are the halogens; and those in 18 are the noble gases.

Exercises

Metal or Nonmetal?

1. Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal:
   1. uranium
   2. bromine
   3. strontium
   4. neon
   5. gold
   6. americium
   7. rhodium
   8. sulfur
   9. carbon
   10. potassium
2. Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal:
   1. cobalt
   2. europium
   3. iodine
   4. indium
   5. lithium
   6. oxygen
   7. cadmium
   8. terbium
   9. rhenium

1. (a) metal, inner transition metal; (b) nonmetal, representative element; (c) metal, representative element; (d) nonmetal, representative element; (e) metal, transition metal; (f) metal, inner transition metal; (g) metal, transition metal; (h) nonmetal, representative element; (i) nonmetal, representative element; (j) metal, representative element

Identifying Elements

1. Using the periodic table, identify the lightest member of each of the following groups:
   1. noble gases
   2. alkaline earth metals
   3. alkali metals
   4. chalcogens
2. Using the periodic table, identify the heaviest member of each of the following groups:
   1. alkali metals
   2. chalcogens
   3. noble gases
   4. alkaline earth metals
3. Use the periodic table to give the name and symbol for each of the following elements:
   1. the noble gas in the same period as germanium
   2. the alkaline earth metal in the same period as selenium
   3. the halogen in the same period as lithium
   4. the chalcogen in the same period as cadmium
4. Use the periodic table to give the name and symbol for each of the following elements:
   1. the halogen in the same period as the alkali metal with 11 protons
   2. the alkaline earth metal in the same period with the neutral noble gas with 18 electrons
   3. the noble gas in the same row as an isotope with 30 neutrons and 25 protons
   4. the noble gas in the same period as gold
5. Write a symbol for each of the following neutral isotopes. Include the atomic number and mass number for each.
   1. the alkali metal with 11 protons and a mass number of 23
   2. the noble gas element with and 75 neutrons in its nucleus and 54 electrons in the neutral atom
   3. the isotope with 33 protons and 40 neutrons in its nucleus
   4. the alkaline earth metal with 88 electrons and 138 neutrons
6. Write a symbol for each of the following neutral isotopes. Include the atomic number and mass number for each.
   1. the chalcogen with a mass number of 125
   2. the halogen whose longest-lived isotope is radioactive
   3. the noble gas, used in lighting, with 10 electrons and 10 neutrons
   4. the lightest alkali metal with three neutrons

Atoms Of Elements That Are In The Same Group Have The Same Number Of What

1. (a) He; (b) Be; (c) Li; (d) O

3. (a) krypton, Kr; (b) calcium, Ca; (c) fluorine, F; (d) tellurium, Te

5. (a) [latex]{}_{11}^{23}text{Na}[/latex] ; (b) [latex]{}_{54}^{129}text{Xe}[/latex] ; (c) [latex]{}_{33}^{73}text{As}[/latex] ; (d) [latex]{}_{88}^{226}text{Ra}[/latex]

Glossary

actinide: inner transition metal in the bottom of the bottom two rows of the periodic table

alkali metal: element in group 1

alkaline earth metal: element in group 2

chalcogen: element in group 16

group: vertical column of the periodic table

halogen: element in group 17

inert gas: (also, noble gas) element in group 18

inner transition metal: (also, lanthanide or actinide) element in the bottom two rows; if in the first row, also called lanthanide, of if in the second row, also called actinide

lanthanide: inner transition metal in the top of the bottom two rows of the periodic table

main-group element: (also, representative element) element in columns 1, 2, and 12–18

metal: element that is shiny, malleable, good conductor of heat and electricity

metalloid: element that conducts heat and electricity moderately well, and possesses some properties of metals and some properties of nonmetals

noble gas: (also, inert gas) element in group 18

nonmetal: element that appears dull, poor conductor of heat and electricity

period: (also, series) horizontal row of the period table

periodic law: properties of the elements are periodic function of their atomic numbers.

periodic table: table of the elements that places elements with similar chemical properties close together

pnictogen: element in group 15

representative element: (also, main-group element) element in columns 1, 2, and 12–18

series: (also, period) horizontal row of the period table

transition metal: element in columns 3–11

Atoms of eight elements A, B, C, D, E, F, G and H have the same number of electron shells but different number of electrons in their outermost shells. It was found that elements A and G combine to form an ionic compound. This ionic compound is added in a small amount to almost all vegetables and dishes during cooking. Oxides of elements A and B are basis in nature while those of elements E and F acidic. The oxide of element D is, however, almost neutral. Based on the above information, answer the following questions:
(a) To which group or period of the periodic table do these elements belong?
(b) What would be the nature of compound formed by a combination of elements B and F?
(c) Which two of these elements could definitely be metals?
(d) Which one of the eight elements is most likely to be found in gaseous state at room temperature?
(e) If the number of electrons in the outermost shell of elements C and G be 3 and 7 respectively, write formula of the compound formed by the combination of C and G.

Solution

(a) The elements belong to the third period of the periodic table, and have the same number of electron shells but different number of electrons in their outermost shells. The number of valence electrons in these elements increases from 1 to 8, on moving from left to right in this period.

(b) When metal B combines with a non-metal F, an ionic compound is formed due to the transfer of electrons from the metal to the non-metal. This is because in the third period, elements A, B and C are metals, D is a metalliod, and E, F, G and H are non-metals.
(c) A and B are definitely metals because in the 3^rd period, at the extreme left, only metals are placed in the periodic table .

(d) The element H is most likely to be found in a gaseous state at room temperature. This is because the last group elements in the periodic table are all in a gaseous state at room tempearture.

(e) If the number of valence electrons of element C is 3 and those of element G is 7, then 1 atom of element C will combine with 3 atoms of element G to form a compound with the formula CG₃.

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