How to Read Element on Periodic Table
Core Concepts:
In this tutorial, you lot will learn how to read the periodic table. We will accept a close look at the groups of the periodic table. In addition, you will learn about the unlike properties of the periodic tabular array groups, periods, and families. If yous enjoy this article, exist 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 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 have the same number of valence electrons and therefore like properties.
The Periodic Tabular array and the Periodic Trends
The periodic tabular array is organized into groups (vertical columns), periods (horizontal rows), and families (groups of elements that are like). Elements in the aforementioned group accept the same number of valence electrons. Meanwhile, elements in the same period have the same number of occupied electron shells. In 1869 Russian chemist Dmitri Mendeleev noticed there existed an innate pattern of organization for the chemic elements. From this deduction, he formed the periodic table. It is important to annotation how the location of elements on this table tells us about their properties. A quick mode to understand an element's chemical and physical backdrop is to know the periodic trends. These trends tell you lot where the highest and lowest types of properties are full-bodied on the periodic table. For a more in-depth explanation of periodic trends, click here.
Group vs Period
Groups are the columns of the periodic table, and periods are the rows. At that place are 18 groups, and at that place are seven periods plus the lanthanides and actinides.
Periods on the Periodic Table
So what is a period on the periodic table? Periods are the horizontal rows of the periodic tabular array. There are seven periods total and each chemical element in a period has the same number of diminutive orbitals. The top period, which contains hydrogen and helium, has just 2 orbitals. Equally you go downwards the rows, the number of orbitals increases. Beneath is a tabular array to help visuals the periodic number and the corresponding orbitals.
| Period Number | Number of Orbitals | Number of Elements |
| ane | 1 | two |
| 2 | two | eight |
| 3 | 3 | 8 |
| 4 | 4 | 18 |
| five | 5 | 18 |
| vi | half dozen | 32 |
| 7 | seven | 32 |
Groups of the Periodic Table
Equally previously mentioned, the vertical columns on the periodic table are called "groups". At that place is eighteen groups on the periodic table in total, and each periodic table group contains elements with the same number of valence electrons.
The number of valence electrons present dictates the backdrop of an chemical element. The reason for this is that the valence electrons, which are the electrons in the outermost shell, are the ones taking part in chemic reactions. These electrons are either donating, accepting, or sharing. Moreover, the more filled the valence shell is, the more than stable the element.
How many groups are in the periodic table?
In that location are xviii groups in the periodic tabular array, one per each column of the periodic tabular array. The starting time column on the left is grouping i, and the last cavalcade on the right is group eighteen.
Groups and Valence Electrons
The start group is the least stable as it only has one valence electron. Meanwhile, grouping xviii is the most stable every bit these elements have a full valence shell (viii valence electrons). Below is a table relating the group numbers to the number of valence electrons.
| Group Number | Number of Valence Electrons |
| 1 | one |
| ii | 2 |
| three-12 | two |
| 13 | 3 |
| fourteen | iv |
| 15 | five |
| 16 | 6 |
| 17 | vii |
| xviii | 8 |
Families of the Periodic Table
On the periodic tabular array, there are families which are groups of elements with like properties. These families are alkali metals, alkaline earth metals, transition metals, post-transition metals, metalloids, halogens, noble metals, and noble gases. Many of these families belong to a single group on the periodic tabular array. Notwithstanding, not all of the families overlap with periodic table groups. For example, the transition metals comprise all elements from group three to group twelve. Below is a periodic table where displaying the location of each family unit.
The Alkali Metals (Group 1)
The alkali 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 usually establish in compounds. In addition, they are water-sensitive (they react violently with water), so they must be stored in oil. The nigh reactive alkali metal is francium and it decreases as you go up the group. This means lithium is the to the lowest degree reactive. Physically, the alkali metallic family is silvery, white, and lite. They also have depression melting and low boiling points.
The Alkaline Globe Metals (Grouping ii)
The alkaline earth metals are the second most reactive family on the periodic table (following backside the alkali metals). Moreover, they are strong reducing agents which means they donate electrons in chemic reactions. They are besides proficient thermal and electrical conductors. Physically, they have low density, low melting point, and a low boiling point.
Rare Earth Metals: Lanthanides
Lanthanides are a family of rare earth metals that contain i valence electron in the 5d shell. They are highly reactive and a strong 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 World Metals: Actinides
Actinides are some other family of rare world metals. Like the lanthanides, these elements are highly reactive. They likewise have loftier electropositivity and are radioactive. Additionally, these elements contain paramagnetic, pyromorphic, and allotropic properties. Physically, they are very similar to lanthanides. They are silver metals that are soft, malleable, and ductile.
The Transition Metals (Groups 3-11)
The transition metals typically form two or more oxidation states. They have low ionization energies and loftier conductivity. In addition, they take loftier melting points, high boiling points, and high conductivity. Physically they are both metallic and malleable.
Post Transition element
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 accept a high density as well equally high conductivity. Physically they are malleable and ductile.
The Metalloids
The metalloids brandish properties of both metals and non-metals. For example, metals are skilful conductors and not-metals are poor conductors. This ways metalloids are semiconductors (only conducts electricity at high temperatures.). Too, they are more breakable than metals but less brittle than non-metals. Physically they can be either shiny or ho-hum and are typically ductile and malleable.
The Halogens (Group 17)
The name element of group vii means "common salt formers" in greek. This is evident in nature as halogens interact with metals to form diverse salts. On another note, the halogens are a unique grouping of elements. They are the only periodic family unit that contains elements in the three states of matter at standard temperature. In that location 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 consummate valence shell. In add-on, noble metals have catalytic tendencies. Likewise, they are very resistant to corrosion, tarnishing, and oxidation. Finally, similar many of the other metals, they are soft and ductile.
Noble Gases (Group xviii)
The noble gases, also called aerogens, are inert gases. Some examples include argon, krypton, and neon. They can be found in group eighteen on the periodic tabular array. Likewise, this means they have a consummate valence beat out. 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 olfactory property.
Summary Table for Family Properties
| Family unit Type | Properties |
| Alkali Metals | – highly reactive – h2o-sensitive – Soft – low density – low melting point – low boiling point |
| Alkali metal Earth Metals | – Strong reducing agents – Silvery, shiny metallic – Good conductors – Low density – Low melting betoken – Low boiling point |
| Transition Metals | – 2 or more oxidation states – Usually forms paramagnetic compounds – Depression ionization energies – High melting point – High boiling point – Loftier conductivity – Metallic – Malleable |
| Post Transition Metals | – Solid at standard temperature – Malleable – Ductile – Loftier conductivity – Loftier density |
| Metalloids | – Semi-conductors (conducts only at high temperatures) – More brittle than metals but less brittle than not-metals – Properties are a mix betwixt metals and non-metals – Shiny or dull – Ductile and malleable |
| Lanthanides | – ane valence electron in 5d shell – Highly reactive – Strong reducing agent – Argent brilliant metal – Relatively soft – Loftier melting points – High boiling points |
| Actinides | – Highly reactive – High electropositivity – Paramagnetic – Pyromorphic – Allotropic – Radioactive – Silvery metals – Ductile – Malleable – Soft |
| Halogens | – Highly reactive – Loftier electronegativity – Not-metal – Toxic |
| Noble Metals | – Relatively unreactive – Complete valence shell (8 valence electrons) – Inert – Catalytic – Resistant to corrosion, tarnishing, and oxidation – Soft and Ductile |
| Noble Gases | – Relatively unreactive – Complete valence vanquish (8 valence electrons) – Low electronegativity – Colorless and odorless – gases under standard weather condition – Non-metallic – Low boiling point – Low melting point – Density increases as yous go down |
Farther Reading
The Structure of an Atom
Periodic Trends Made Easy!
Source: https://chemistrytalk.org/how-to-read-the-periodic-table/
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