How Many Families Are There on the Periodic Table?
Cadre Concepts:
In this tutorial, y'all will learn how to read the periodic table. We will take a close look at the groups of the periodic table. In addition, you will acquire about the dissimilar properties of the periodic table groups, periods, and families. If y'all enjoy this article, be sure to check out our others!
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Vocabulary
- Elements: A pure substance composed of a single atom.
- Groups: The vertical column of the periodic tabular array that signifies the number of valence electrons in an element.
- Periods: The horizontal rows in the periodic table that signify the number of electron shells in an element.
- Families: Elements that accept the same number of valence electrons and therefore similar properties.
The Periodic Table and the Periodic Trends
The periodic table is organized into groups (vertical columns), periods (horizontal rows), and families (groups of elements that are similar). Elements in the same grouping have the same number of valence electrons. Meanwhile, elements in the same menstruum have the same number of occupied electron shells. In 1869 Russian chemist Dmitri Mendeleev noticed there existed an innate blueprint of organization for the chemic elements. From this deduction, he formed the periodic tabular array. It is important to note how the location of elements on this tabular array tells us about their backdrop. A quick manner to sympathize an element's chemical and physical properties is to know the periodic trends. These trends tell you where the highest and everyman types of properties are full-bodied on the periodic tabular array. For a more in-depth caption of periodic trends, click hither.
Group vs Period
Groups are the columns of the periodic table, and periods are the rows. There are xviii groups, and in that location are 7 periods plus the lanthanides and actinides.
Periods on the Periodic Tabular array
Then what is a period on the periodic table? Periods are the horizontal rows of the periodic table. There are seven periods full and each element in a period has the same number of atomic orbitals. The top period, which contains hydrogen and helium, has only two orbitals. Every bit you go down the rows, the number of orbitals increases. Beneath is a table to help visuals the periodic number and the corresponding orbitals.
| Period Number | Number of Orbitals | Number of Elements |
| i | one | 2 |
| 2 | two | 8 |
| 3 | iii | 8 |
| iv | 4 | xviii |
| five | 5 | 18 |
| 6 | 6 | 32 |
| 7 | 7 | 32 |
Groups of the Periodic Table
As previously mentioned, the vertical columns on the periodic table are called "groups". There is 18 groups on the periodic tabular array in total, and each periodic table group contains elements with the aforementioned number of valence electrons.
The number of valence electrons present dictates the properties of an element. The reason for this is that the valence electrons, which are the electrons in the outermost shell, are the ones taking part in chemical reactions. These electrons are either donating, accepting, or sharing. Moreover, the more filled the valence shell is, the more stable the element.
How many groups are in the periodic table?
There are xviii groups in the periodic table, one per each cavalcade of the periodic tabular array. The beginning cavalcade on the left is group 1, and the final column on the correct is grouping 18.
Groups and Valence Electrons
The starting time grouping is the least stable as information technology only has one valence electron. Meanwhile, group eighteen is the most stable as these elements have a full valence shell (8 valence electrons). Below is a tabular array relating the grouping numbers to the number of valence electrons.
| Grouping Number | Number of Valence Electrons |
| i | 1 |
| ii | 2 |
| three-12 | two |
| 13 | iii |
| fourteen | iv |
| 15 | 5 |
| 16 | half-dozen |
| 17 | 7 |
| 18 | 8 |
Families of the Periodic Tabular array
On the periodic table, there are families which are groups of elements with similar properties. These families are brine metals, alkali metal earth metals, transition metals, mail-transition metals, metalloids, halogens, noble metals, and noble gases. Many of these families vest to a single grouping on the periodic table. Yet, not all of the families overlap with periodic table groups. For example, the transition metals contain all elements from grouping three to group twelve. Below is a periodic table where displaying the location of each family unit.
The Alkali Metals (Group one)
The brine metals consist of all of the elements in group one with the exception of hydrogen. These elements are extremely reactive and for this reason, are ordinarily institute in compounds. In addition, they are water-sensitive (they react violently with water), and so they must be stored in oil. The near reactive element of group i is francium and it decreases equally you become up the group. This means lithium is the to the lowest degree reactive. Physically, the element of group i family is silvery, white, and light. They also have low melting and low humid points.
The Alkaline Earth Metals (Group two)
The alkaline globe metals are the 2nd most reactive family on the periodic table (following behind the alkali metals). Moreover, they are stiff reducing agents which means they donate electrons in chemical reactions. They are also skilful thermal and electric conductors. Physically, they have low density, low melting point, and a low humid signal.
Rare World Metals: Lanthanides
Lanthanides are a family of rare earth metals that contain 1 valence electron in the 5d trounce. They are highly reactive and a strong reducing agent in reactions. Furthermore, they are a silver-bright metal and are relatively soft. They also have both high melting points and high boiling points. The rare earths include elements like neodymium and erbium.
Rare Earth Metals: Actinides
Actinides are another family of rare globe metals. Like the lanthanides, these elements are highly reactive. They also take high electropositivity and are radioactive. Additionally, these elements contain paramagnetic, pyromorphic, and allotropic properties. Physically, they are very like to lanthanides. They are argent metals that are soft, malleable, and ductile.
The Transition Metals (Groups 3-11)
The transition metals typically grade ii or more than oxidation states. They have low ionization energies and high conductivity. In addition, they accept high melting points, high boiling points, and high conductivity. Physically they are both metal and malleable.
Post Transition Metal
The post transition metals are located in betwixt the transition metals and the metalloids. At standard temperature, they are in a solid state of thing. They tend to have a high density likewise every bit high electrical conductivity. Physically they are malleable and ductile.
The Metalloids
The metalloids brandish properties of both metals and non-metals. For example, metals are good conductors and non-metals are poor conductors. This means metalloids are semiconductors (but conducts electricity at high temperatures.). Also, they are more than brittle than metals but less brittle than not-metals. Physically they can be either shiny or dull and are typically ductile and malleable.
The Halogens (Group 17)
The name halogen ways "common salt formers" in greek. This is evident in nature as halogens interact with metals to form various salts. On another note, the halogens are a unique group of elements. They are the only periodic family that contains elements in the three states of matter at standard temperature. There are 6 halogens and they are located in group 17. These elements include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). They are highly reactive, highly electronegative, and highly toxic non-metals.
Noble Metals
The noble metals consist of ruthenium (Ru), osmium (Os), rhodium (Rh), iridium (Ir), Pd, platinum (Pt), gold (Au), argent (Ag). Like the noble gases, they are inert due to having a complete valence shell. In addition, noble metals have catalytic tendencies. Also, they are very resistant to corrosion, tarnishing, and oxidation. Finally, like many of the other metals, they are soft and ductile.
Noble Gases (Group 18)
The noble gases, too called aerogens, are inert gases. Some examples include argon, krypton, and neon. They can be found in group 18 on the periodic tabular array. As well, this means they have a complete valence vanquish. For this reason, they are stable and relatively unreactive. Furthermore, the noble gases have low boiling points and low melting points. Physically they are colorless and have no smell.
Summary Table for Family Properties
| Family unit Blazon | Properties |
| Alkali Metals | – highly reactive – h2o-sensitive – Soft – low density – low melting signal – low boiling indicate |
| Element of group i Earth Metals | – Strong reducing agents – Silvery, shiny metallic – Good conductors – Depression density – Low melting point – Low boiling indicate |
| Transition Metals | – ii or more oxidation states – Unremarkably forms paramagnetic compounds – Low ionization energies – High melting point – High humid point – High conductivity – Metal – Malleable |
| Post Transition Metals | – Solid at standard temperature – Malleable – Ductile – Loftier conductivity – Loftier density |
| Metalloids | – Semi-conductors (conducts merely at loftier temperatures) – More brittle than metals but less brittle than non-metals – Properties are a mix betwixt metals and non-metals – Shiny or dull – Ductile and malleable |
| Lanthanides | – 1 valence electron in 5d shell – Highly reactive – Strong reducing agent – Argent vivid metallic – Relatively soft – High melting points – High boiling points |
| Actinides | – Highly reactive – Loftier electropositivity – Paramagnetic – Pyromorphic – Allotropic – Radioactive – Silver metals – Ductile – Malleable – Soft |
| Halogens | – Highly reactive – Loftier electronegativity – Non-metal – Toxic |
| Noble Metals | – Relatively unreactive – Complete valence beat out (8 valence electrons) – Inert – Catalytic – Resistant to corrosion, tarnishing, and oxidation – Soft and Ductile |
| Noble Gases | – Relatively unreactive – Consummate valence shell (eight valence electrons) – Depression electronegativity – Colorless and odorless – gases under standard atmospheric condition – Non-metal – Depression humid signal – Low melting point – Density increases as you go down |
Further Reading
The Structure of an Atom
Periodic Trends Made Like shooting fish in a barrel!
Source: https://chemistrytalk.org/how-to-read-the-periodic-table/
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