How Can You Identify the Elements in a Family on the Periodic Table?
Core Concepts:
In this tutorial, you will learn how to read the periodic tabular array. We will take a close look at the groups of the periodic table. In addition, you lot will learn about the different properties of the periodic table groups, periods, and families. If y'all bask this commodity, be sure to check out our others!
Related Manufactures:
- Periodic Trends Fabricated Easy
- Elements
- How to Write Electron Shell Configurations
- Atomic Radius Trend
- Ionization Energy Tendency
Vocabulary
- Elements: A pure substance composed of a single atom.
- Groups: The vertical column of the periodic table 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 chemical element.
- Families: Elements that accept the aforementioned 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 group have the same number of valence electrons. Meanwhile, elements in the same period accept the same number of occupied electron shells. In 1869 Russian pharmacist Dmitri Mendeleev noticed there existed an innate blueprint of organisation for the chemical elements. From this deduction, he formed the periodic table. It is important to note how the location of elements on this table tells united states about their properties. A quick way to understand an element's chemical and concrete properties is to know the periodic trends. These trends tell you lot where the highest and lowest types of properties are concentrated on the periodic table. For a more in-depth explanation of periodic trends, click here.
Group vs Menstruum
Groups are the columns of the periodic table, and periods are the rows. There are 18 groups, and there are 7 periods plus the lanthanides and actinides.
Periods on the Periodic Table
So what is a catamenia on the periodic table? Periods are the horizontal rows of the periodic tabular array. In that location are seven periods total and each element in a period has the aforementioned number of atomic orbitals. The top flow, which contains hydrogen and helium, has only 2 orbitals. As you go down the rows, the number of orbitals increases. Below is a table to assist visuals the periodic number and the corresponding orbitals.
| Flow Number | Number of Orbitals | Number of Elements |
| one | ane | 2 |
| two | 2 | 8 |
| three | 3 | eight |
| four | 4 | 18 |
| v | 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". In that location is eighteen groups on the periodic tabular array in total, and each periodic tabular array group contains elements with the same number of valence electrons.
The number of valence electrons present dictates the properties of an chemical element. The reason for this is that the valence electrons, which are the electrons in the outermost vanquish, are the ones taking role in chemic reactions. These electrons are either donating, accepting, or sharing. Moreover, the more filled the valence shell is, the more than stable the chemical element.
How many groups are in the periodic tabular array?
There are xviii groups in the periodic table, 1 per each column of the periodic table. The get-go cavalcade on the left is group 1, and the final column on the right is group 18.
Groups and Valence Electrons
The first group is the to the lowest degree stable as it just has one valence electron. Meanwhile, group eighteen is the nearly stable as these elements take a full valence shell (eight valence electrons). Beneath is a table relating the grouping numbers to the number of valence electrons.
| Grouping Number | Number of Valence Electrons |
| 1 | 1 |
| 2 | 2 |
| 3-12 | 2 |
| 13 | 3 |
| 14 | iv |
| xv | 5 |
| 16 | 6 |
| 17 | 7 |
| 18 | eight |
Families of the Periodic Table
On the periodic table, there are families which are groups of elements with similar properties. These families are alkali metals, alkaline globe metals, transition metals, post-transition metals, metalloids, halogens, noble metals, and noble gases. Many of these families belong to a single grouping on the periodic table. However, non all of the families overlap with periodic table groups. For example, the transition metals contain all elements from group three to group twelve. Beneath is a periodic table where displaying the location of each family unit.
The Alkali Metals (Grouping one)
The brine metals consist of all of the elements in group ane with the exception of hydrogen. These elements are extremely reactive and for this reason, are usually institute in compounds. In addition, they are water-sensitive (they react violently with h2o), so they must be stored in oil. The most reactive alkali metal is francium and it decreases as you get up the group. This means lithium is the least reactive. Physically, the alkali metal family is silvery, white, and light. They also have depression melting and depression humid points.
The Alkaline Earth Metals (Group 2)
The alkaline earth metals are the 2d almost reactive family unit on the periodic table (post-obit backside the alkali metals). Moreover, they are strong reducing agents which means they donate electrons in chemical reactions. They are also practiced thermal and electrical conductors. Physically, they have depression density, low melting point, and a low humid point.
Rare Earth Metals: Lanthanides
Lanthanides are a family unit of rare earth metals that contain one valence electron in the 5d shell. They are highly reactive and a stiff reducing agent in reactions. Furthermore, they are a silvery-brilliant 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 unit of rare world metals. Similar the lanthanides, these elements are highly reactive. They also have high electropositivity and are radioactive. Additionally, these elements contain paramagnetic, pyromorphic, and allotropic backdrop. Physically, they are very similar to lanthanides. They are silvery metals that are soft, malleable, and ductile.
The Transition Metals (Groups 3-11)
The transition metals typically form ii or more than oxidation states. They have low ionization energies and high conductivity. In improver, they have high melting points, loftier boiling points, and high conductivity. Physically they are both metallic and malleable.
Post Transition Metallic
The post transition metals are located in between the transition metals and the metalloids. At standard temperature, they are in a solid state of matter. They tend to have a loftier density also as high conductivity. Physically they are malleable and ductile.
The Metalloids
The metalloids display backdrop of both metals and non-metals. For example, metals are expert conductors and non-metals are poor conductors. This means metalloids are semiconductors (only conducts electricity at high temperatures.). Also, they are more brittle than metals but less brittle than non-metals. Physically they can be either shiny or boring and are typically ductile and malleable.
The Halogens (Group 17)
The proper noun halogen ways "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 affair at standard temperature. In that location are 6 halogens and they are located in grouping 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), silvery (Ag). Like the noble gases, they are inert due to having a complete valence vanquish. In improver, noble metals accept catalytic tendencies. As well, 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, also chosen aerogens, are inert gases. Some examples include argon, krypton, and neon. They tin be establish in grouping eighteen on the periodic table. Also, this means they have a consummate valence crush. For this reason, they are stable and relatively unreactive. Furthermore, the noble gases have low humid points and low melting points. Physically they are colorless and have no olfactory property.
Summary Table for Family unit Properties
| Family Type | Properties |
| Alkali Metals | – highly reactive – h2o-sensitive – Soft – depression density – low melting point – low boiling point |
| Alkaline metal Globe Metals | – Strong reducing agents – Silvery, shiny metal – Good conductors – Depression density – Low melting signal – Depression boiling signal |
| Transition Metals | – 2 or more than oxidation states – Unremarkably forms paramagnetic compounds – Low ionization energies – High melting bespeak – High boiling point – Loftier electrical conductivity – Metal – Malleable |
| Post Transition Metals | – Solid at standard temperature – Malleable – Ductile – Loftier conductivity – High density |
| Metalloids | – Semi-conductors (conducts but at high temperatures) – More brittle than metals simply less brittle than non-metals – Properties are a mix between metals and non-metals – Shiny or tiresome – Ductile and malleable |
| Lanthanides | – 1 valence electron in 5d shell – Highly reactive – Potent reducing agent – Silvery bright metal – Relatively soft – High melting points – High humid points |
| Actinides | – Highly reactive – High electropositivity – Paramagnetic – Pyromorphic – Allotropic – Radioactive – Silver metals – Ductile – Malleable – Soft |
| Halogens | – Highly reactive – High electronegativity – Non-metal – Toxic |
| Noble Metals | – Relatively unreactive – Consummate valence beat out (8 valence electrons) – Inert – Catalytic – Resistant to corrosion, tarnishing, and oxidation – Soft and Ductile |
| Noble Gases | – Relatively unreactive – Complete valence trounce (8 valence electrons) – Low electronegativity – Colorless and odorless – gases nether standard conditions – Non-metallic – Low boiling point – Depression melting point – Density increases equally yous become down |
Further Reading
The Structure of an Atom
Periodic Trends Fabricated Easy!
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Source: https://chemistrytalk.org/how-to-read-the-periodic-table/
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