Where Are the Inert Gases on Periodic Table

With the introduction of electron configurations, we began to get a deeper understanding of the Periodic Prorogue. An understanding of these electron configurations will testify to be invaluable Eastern Samoa we look at soldering and chemical reactions. The orbital representation method for representing electron configuration is shown below. The orbital representation was learned in an earlier chapter but comparable more of the skills you check in chemistry, IT will be used a great whole slew in this chapter and in individual chapters ulterior in the course.

In this lesson, we will center on the association between the negatron configuration and the main group elements of the Periodic Table. We will need to remember the sub-level fill groups in the Periodic Table. Keep the following figure in mind. We will wont it for the next two chapters.

Lesson Objectives [edit | edit source]

• Describe the patterns that exist in the electron configurations for the chief group elements.
• Identify the columns in the Periodic Table that contain 1) the base metals, 2) the alkaline earth metals, 3) the halogens, and 4) the noble gases, and describe the differences betwixt for each one family's electron configuration.
• Given the outermost energy state electron configuration for an element, determine its family on the Oscillating Table.

Alkali Metals Have One Electron in Their Outer Energy Tier [edit | edit out source]

Elements Ending with s ¹ = Base

In the Periodic Set back, the elements are arranged in ordinate of flaring microscopic come. In previous reincarnate we learned that the substance number is the issue of protons in the nucleus of an atom. For a neutral atom, the turn of protons is equal to the number of electrons. Therefore, for neutral atoms, the Rhythmical Prorogue is also arranged in edict of increasing number of electrons. Get a load at present at the front group Beaver State column in the Periodic Hold over. IT is the one marked "1A" in the Historic period Table figure above. The groups Beaver State families are the vertical rows of elements. The first radical has seven elements representing the septenar periods of the Oscillating Table. Remember that a flow in the Periodic Put of is a level row. Group 1A is the lone group with seven elements in it.

Postpone 9.1: Electron Configurations for Group 1A Metals

Element	Minute Number	Electron Configuration
Lithium (Li)	3	${\displaystyle 1s^{2}2s^{1}}$
Na (Na)	11	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{1}}$
Potassium (K)	19	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}}$
Rb (Rb)	37	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{1}}$
Cesium (Cs)	55	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{1}}$
Francium (Fr)	87	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{1}}$

Table 9.1: Negatron Configurations for Radical 1A Metals

Element	Matter Identification number	Electron Form
Atomic number 3 (Fifty-one)	3	${\displaystyle 1s^{2}2s^{1}}$
Sodium (Na)	11	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{1}}$
Potassium (K)	19	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}}$
Rubidium (Rb)	37	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{1}}$
Cesium (Atomic number 55)	55	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{1}}$
Francium (Fr)	87	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{1}}$

What do you notice about all of the elements in Group 1? They all have s ¹ as the outermost energy state electron configuration. The whole number before of the "s" tells you what period the element is in. For example sodium, Na, has the electron configuration 1s ²2s ²2p ⁶3s ¹, so it is in period 3. Information technology is the prime element of this period.

This group of elements is called the alkali metals. They get their name from ancient Arabic language (al barilla) because "scientists" of the clock time found that the ashes of the flora they were burning contained a large amount of Na and potassium. In Arabic, al barilla way ashes. We know now that all alkali metals have electronic configurations ending in s ¹. You might want to note that spell hydrogen is ofttimes placed in group 1, it is not considered an alkali metal. The reason for this will be discussed later.

Alkaline Earth Elements Have Two Electrons in Their Out Vitality Level [edit | delete rootage]

Elements Ending with s ² = Alkaline-earth metal

Taking a look at Aggroup 2A in Put of 9.2, we can use the equal analysis we used with aggroup 1 to check if we can find a corresponding course. It is the second vertical group in the Periodic Postpone and information technology contains only six elements.

Table 9.2: Electron Configurations for Group 2A Metals

Element	Matter Amoun	Electron Shape
Beryllium (Be)	4	${\displaystyle 1s^{2}2s^{2}}$
Mg (Mg)	12	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}}$
Calcium (Ca)	20	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}}$
Sr (Sr)	38	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}}$
Barium (Ba)	56	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}}$
Radium (Ra)	88	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}}$

Table 9.2: Negatron Configurations for Group 2A Metals

Element	Atomic Number	Negatron Conformation
Be (Be)	4	${\displaystyle 1s^{2}2s^{2}}$
Magnesium (Mg)	12	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}}$
Calcium (Ca)	20	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}}$
Strontium (Sr)	38	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}}$
Barium (Ba)	56	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}}$
Radium (Ra)	88	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}}$

What coif you notice about all of the elements in aggroup 2A? They altogether undergo an outermost energy level electron configuration of s ². The whole number in front of the "s" tells you what menstruum the element is in. For example, atomic number 12, Mg, has the negatron configuration 1s ²2s ²2p ⁶3s ², so it is in period 3 and is the second element in that time period. Remember that the s sublevel whitethorn clutch two electrons, so in Radical 2A, the s orbital has been filled.

Elements in this group are given the name alkaline earth metals. They let their name because early "scientists" found that all of the alkaline earths were found in the earth's impertinence. Alkaline-earth metal metals, although not as reactive as the alkali metals, are still extremely unstable. All alkaline earth metals have electron configurations ending in s ².

Noble Gases Have 8 Electrons in Their Outer Vitality Level [edit | edit source]

Elements Ending with s ² p ⁶ = Noble Gases

The first person to isolate a noble gas was H Cavendish, who disjunct Ar in the late 1700s. The noble gases were in reality considered inert gases until the 1960s when a compound was rudder-like between atomic number 54 and fluorine which changed the way chemists viewed the "inert" gases. In the European country language, soggy means to be lifeless operating room motionless; in the chemical world, neutral means does not react. Late, the name "imposing gasoline" replaced "unreactive gas" for the name of Radical 8A.

When we write out the electron configurations for these elements, we hear the same general trend that was observed with groups 1A and 2A; that is, similar electron configurations inside the group.

Tabular array 9.3: Electron Configurations for Group 8A Gases

Element	Atomic Number	Electron Configuration
Helium (He)	2	${\displaystyle 1s^{2}}$
Atomic number 10 (Ne)	10	${\displaystyle 1s^{2}2s^{2}2p^{6}}$
Argon (Ar)	18	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}}$
Krypton (Kr)	36	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}}$
Xenon (Xe)	54	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}}$
Radon (Rn)	86	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}}$

Table 9.3: Electron Configurations for Group 8A Gases

Element	Atomic Number	Negatron Constellation
Helium (He)	2	${\displaystyle 1s^{2}}$
Atomic number 10 (Nebraska)	10	${\displaystyle 1s^{2}2s^{2}2p^{6}}$
Atomic number 18 (Ar)	28	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}}$
Krypton (Kr)	36	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}}$
Xe (Xe)	54	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}}$
Radon (Rn)	86	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}}$

Aside from helium, He, each of the noble gases have outer energy state electron configurations that are the same, ns ² Np ⁶, where n is the period count. So Argon, Ar, is in period 3, is a inert gas, and would therefore have an outer energy level negatron configuration of 3s ²3p ⁶. Notice that both the s and p sublevels are filled. Atomic number 2 has an negatron contour that might fit into Group 2A. Even so, the chemic responsiveness of helium, because it has a full first energy level, is similar to that of the noble gases.

Halogens Give birth 7 Electrons in Their Outer Energy state [edit | edit source]

Elements Finish with s ² p ⁵ = Halogens

The halogens are an interesting group. Halogens are members of Group 7A, which is also referred to as 17. It is the only mathematical group in the Periodic Table that contains all of the states of matter at room temperature. Fluorine, F₂, is a gas, every bit is chlorine, Cl₂. Br, Red Brigades₂, is a swimming and iodine, I₂, and atomic number 85, At₂, are both solids. What else is neat about Group 7A is that it houses tetrad (4) of the seven (7) diatomic compounds. Think back the diatomics are H₂, N₂, O₂, F₂, Cl₂, Br₂, and I₂. Notice that the latter four are Mathematical group 17 elements. The word halogen comes from the Greek meaning salt forming. French chemists discovered that the majority of halogen ions will form salts when combined with metals. We all know about of these already: LiF, NaCl, KBr, and NaI.

Fetching a facial expression at Group 7A in the figure, we can find the synoptical pattern of similar negatron configurations as found with group 1A, 2A, and 8A. It is the 17^{atomic number 90} grouping in the Periodic Table and IT contains only cinque elements.

Table 9.4: Electron Configurations for Grouping 7A Elements

Element	Atomic Number	Electron Configuration
Fluorine (F)	9	${\displaystyle 1s^{2}2s^{2}2p^{5}}$
Chlorine (One hundred fifty)	17	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}}$
Bromine (Br)	35	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}}$
Iodine (I)	53	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{5}}$
Astatine (At)	85	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{5}}$

Set back 9.4: Negatron Configurations for Group 7A Elements

Element	Atomic Number	Electron Configuration
Fluorine (F)	9	${\displaystyle 1s^{2}2s^{2}2p^{5}}$
Chlorine (Cl)	17	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}}$
Atomic number 35 (Atomic number 35)	35	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}}$
Iodine (I)	53	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{5}}$
Astatine (At)	85	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{5}}$

What is the general vogue for the elements in Group 7A? They all have, As the outermost energy storey negatron configuration, ns ² np ⁵, where n is the period number. You should besides note that these elements are one group away from the noble gases (the ones that generally don't react!) and the outermost electron configuration of the halogens is incomparable away from being filled. For example, chlorine (Cl) has the electron configuration [NE] 3s ²3p ⁵ so it is in period 3, the seventh element in the main group elements. The main group elements, every bit you recall, are tantamount to the s + p blocks of the Periodic Table (or the pink and orange groups in the diagram supra).

The Oxygen Fellowship Has 6 Electrons in the Outermost Energy Level [delete | edit source]

Elements Ending with s ² p ⁴ = the Oxygen Family

Oxygen and the other elements in Group 6A have a similar trend in their electron configurations. Atomic number 8 is the only gas in the group; all others are in the solid state at room temperature. Oxygen was first named away Antoine Lavoisier in the late 1700s but real the major planet has had oxygen around since plants were first on the solid ground.

Taking a look at Group 6A in the build below, we find the same pattern in electron configurations that we found with the opposite groups. Oxygen and its folk members are in the 16^th group in the Periodic Table. In Aggroup 16, at that place are, again, just five elements.

Table 9.5: Electron Configurations for Group 6A Elements

Constituent	Microscopical Number	Negatron Conformation
Oxygen (O)	8	${\displaystyle 1s^{2}2s^{2}2p^{4}}$
Sulfur (S)	16	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}}$
Selenium (Southeastward)	34	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{4}}$
Atomic number 52 (Te)	52	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{4}}$
Po (Petty officer)	84	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{4}}$

Table 9.5: Electron Configurations for Mathematical group 6A Elements

Chemical element	Atomic Number	Electron Configuration
Oxygen (O)	8	${\displaystyle 1s^{2}2s^{2}2p^{4}}$
S (S)	16	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}}$
Selenium (Se)	34	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{4}}$
Tellurium (Te)	52	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{4}}$
Polonium (Po)	84	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{4}}$

When we analyse the electron configurations of the Aggroup 6A elements, we ensure that wholly of these elements have the outer energy level electron form of ns ² np ⁴. We will assure that this like negatron configuration gives all elements in the group corresponding properties for bonding.

These elements are two groups gone from the exalted gases and the outermost electron shape is two inaccurate from beingness filled. Sulfur, for instance, has the electron configuration 1s ²2s ²2p ⁶3s ²3p ⁴ indeed it is in period 3. Sulfur is the sixth element in the principal group elements. We know it is the 6th chemical element across the catamenia of the independent group elements because there are 6 electrons in the outmost energy level.

The Nitrogen Family Has 5 Electrons in the Outer Energy state [cut | edit source]

Elements Ending with s ² p ³ = the Nitrogen Family

Just equally we saw with Group 6A, Group 5A has a synonymous crotchet in its radical. Nitrogen is the exclusively gas in the group with totally other members in the whole state at room temperature. Nitrogen was prototypic discovered by the European country chemist First Baron Rutherford in the late 1700s. The air is mostly made of nitrogen. N has properties that are different in some shipway from its group members. As we will learn in later lessons, the negatron configuration for nitrogen provides the ability to form very strong triple bonds.

Nitrogen and its family members belong in the 15^th group in the periodic put over. In Group 15, there are also just five elements.

Hold over 9.6: Negatron Configurations for Group 5A Elements

Element	Microscopical Number	Electron Contour
Nitrogen (N)	7	${\displaystyle 1s^{2}2s^{2}2p^{3}}$
Phosphoric (P)	15	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}}$
Ratsban (A)	33	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{3}}$
Antimony (Sb)	51	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{3}}$
Atomic number 83 (Bi)	83	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{3}}$

Table 9.6: Electron Configurations for Group 5A Elements

Element	Atomic Identification number	Electron Configuration
Nitrogen (N)	7	${\displaystyle 1s^{2}2s^{2}2p^{3}}$
Chemical element (P)	15	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}}$
Arsenic (As)	33	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{3}}$
Atomic number 51 (Sb)	51	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{3}}$
Bismuth (Bi)	83	${\displaystyle 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}}$ ${\displaystyle 4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{3}}$

What is the general trend for the elements in group 5A? They all have, Eastern Samoa the electron configuration in the outermost energy level, ns ² np ³, where n is the period number. These elements are triplet groups away from the noble gases and the outer energy state electron configuration is three off from having a completed outer energy level. In other words, the p sublevel in the Group 15 elements is incomplete full. Arsenic, for example, has the negatron shape 1s ²2s ²2p ⁶3s ²3p ⁶4s ²3d ¹⁰4p ³ so it is in menstruum 4, the fifth element in the main group elements. We know it is the fifth element crossways the historical period of the main group elements because on that point are 5 electrons in the outermost energy level.

Moral Summary [redact | edit source]

• Families in the cyclic table are the vertical columns and are also referred to Eastern Samoa groups.
• Group 1A elements are the alkali metals and all have one negatron in the outer energy level because their electron configuration ends in s ¹.
• Mathematical group 2A elements are the alkaline dry land metals and all throw ii electrons in the outermost energy state because their electron configuration ends in s ².
• Group 5A elements all have five electrons in the outermost energy level because their electron configuration ends in s ² p ³.
• Group 6A elements each have six electrons in the outermost energy level because their negatron form ends in s ² p ⁴.
• Group 7A elements are the halogens and all have seven electrons in the outermost energy state because their electron configuration ends in s ² p ⁵.
• Group 8A elements are the monarchical gases and entirely have eight electrons in the outmost vigor level because their electron configuration ends in s ² p ⁶.
• Elements in group 8A get the most stable electron form in the outer shell because the sublevels are completely filled with electrons.

Review Questions [edit | edit informant]

1. If an element is said to have an outermost electronic form of ns ² np ³, it is in what group in the rhythmic table?

   (a) Aggroup 3A

   (b) Group 4A

   (c) Group 5A

   (d) Group 7A

2. What is the general electronic shape for the Group 8A elements? (Bank note: when we wish to indicate an electron configuration without specifying the exact energy tear down, we use the alphabetic character "n" to represent any energy level number. That is, ns ² np ³ represents any of the following; 2s ²2p ³, 3s ²3p ³, 4s ²4p ³, and so on.)

   (a) ns ² np ⁶

   (b) ns ² np ⁵

   (c) ns ² np ¹

   (d) ns ²

3. The grouping 2 elements are given what name?

   (a) alkali metals

   (b) alkaline earth metals

   (c) halogens

   (d) noble gases

4. Using the diagram down the stairs, identify:

   (a) The alkali metal away giving the letter that indicates where the ingredient would be located and write the outermost physics shape.

   (b) The alkaline earth metal past freehanded the letter that indicates where the element would be settled and write out the outermost electronic configuration.

   (c) The noble gas by giving the letter that indicates where the element would be located and write the outermost electronic shape.

   (d) The halogen past giving the varsity letter that indicates where the element would Be located and write the outermost physical science configuration.

   (e) The element with an outermost electronic configuration of s ² p ³ by handsome the letter that indicates where the element would be located.

   (f) The element with an outmost electronic configuration of s ² p ¹ aside giving the letter that indicates where the chemical element would personify located.

   

5. In the oscillatory table, mention the element whose outermost electronic configuration is found below. Where latent, give the name of the group.

   (a) 5s ²

   (b) 4s ²3d ¹⁰4p ¹

   (c) 3s ²3p ³

   (d) 5s ²4d ¹⁰5p ²

   (e) 3s ¹

   (f) 1s ²

   (g) 6s ²5d ¹⁰6p ⁵

   (h) 4s ²4p ⁴

Lexicon [edit | edit informant]

alkali metals

Group 1 in the periodic table (Li, Na, K, Rb, Cesium, Fr).

alkaline earth metals

Group 2 in the periodic table (Be, Magnesium, Ca, Sr, Barium, Ra).

group

Columns of the oscillating table.

halogens

Group 17 in the periodic table (F, Cl, Br, I, At).

independent group elements

Equivalent to the s + p blocks of the periodic postpone, a.k.a. "voice elements".

noble gases

Group 18 in the periodic table (He, Ne, Ar, Kr, Xe, Rn).

period

Horizontal rows of the periodic table.

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Where Are the Inert Gases on Periodic Table

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