Atoms and Reactions

This unit will explore in more detail the structure of atoms and how this structure is key to understanding chemical reactions. Understanding how elements were positioned in the Periodic Table will further underpin the basics of chemistry that is required for students to continue their understanding of the Material World.

THE PERIODIC TABLE & THE FIRST 20 ELEMENTS

The Periodic Table is a way to order the elements according to their different properties. It was first created by Dimitri Mendeleev in 1869 with just 63 elements identified. His original table had 'gaps' left which slowly were filled as the 'missing' elements were discovered.

Periodic Table Quiz - First 20 ElementsCan you guess the first twenty elements of the periodic table?

AtomsView the interactive image by Carrie

See Whether You Know the First 20 Element SymbolsHere's a fun quiz that tests how well you know the first 20 element symbols on the periodic table.

From the first 20 elements - 12 are solids at room temperature and 8 are gases (hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine and argon)
The vertical columns are called Groups
Atoms of elements in the same group have the same number of electrons in their valence shell, so they have similar chemical properties
The horizontal rows are called Periods - Atoms of elements in the same period have the same number of electron shells
Across a period, the number of electrons in the outer shell starts at 1 and then increases by 1 for each element until an outer shell of 8 is reached for the last element on the extreme right-hand side of the row- this element is stable since it has a full outer shell
Each row on the periodic table corresponds to filling a shell of electrons. Hydrogen and helium are the only elements in the first period; they are filling the first shell which holds a maximum of two electrons
Metals are on the left of the table and non-metals are on the right

Uncommon Element Symbols

Na - sodium, from the Latin word for sodium natrium.

K - potassium, from the Latin word for potassium kalium.

Fe - iron, fron the Latin word for iron ferrum.

Cu - copper, from the Latin word for copper cuprum.

Ag - silver, from the Latin word for silver argentum

Sn - tin, from the Latin word for tin stannum

Sb - antimony, from the Latin name for antimony sulfide stibium.

W - tungsten, from the German name for tungsten wolfram.

Au - gold, from the Latin word for gold aurum.

Hg - mercury, from the Latin for liquid silver hydrargyrum.

Pb - lead, from the Latin word for lead plumbum.

PERIODIC TABLE GAME - CLICK ON IT TO PLAY!

The Periodic TableSuitable for grades 6 - 8, Periodic Table Game lets you identify symbols & names of elements. Answer correctly to win. Play Periodic Table Game online, here.

Periodic Table Groups

Group 1: Alkali Metals

Alkali metals are soft, ductile, and good conductors of electricity and heat. This group includes the elements Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium. Alkali metals are very reactive. Compared to other elements they have a low melting and boiling point.

Group 2: Alkaline Earth Metals

The second group of elements in the Periodic table is Alkaline Earth metals. These elements are found in the crust of the earth and are soft and silvery metals. They can conduct heat and electricity and can be made into sheets. Some elements in this group are Beryllium, Calcium, and Magnesium.

Group 3 To Group 12: Transition Metals

The elements from Group 3 to 12 are called Transition Metals. They include the Scandium, Titanium, Vanadium, Chromium, Manganese, Iron, Cobalt, Nickel, Copper, and Zinc families of elements. Transition Metals are hard and dense, are good conductors of heat and electricity, and can be bent easily. Gold, Iron, and Copper are important such elements.

Group 13: Boron Group

The Boron Group is named after the lead element of Boron. They are good conductors but are rarely found in nature. Aluminium is an exception in this group as it is found in abundance.

Group 14: Carbon Group

The Carbon group, consists of Carbon, Silicon, Germanium, Tin, Lead, and Flerovium. All the elements are found in nature quite widely, except Flerovium. Elements in this group and their compounds are usually toxic.

Group 15: Pnictogens

The Pnictogens are made of Nitrogen (N), followed by Phosphorus (represented as P), Arsenic (As), Antimony (Sb), Bismuth (Bi), and finally, Moscovium (Mc). While Nitrogen and Phosphorus are found naturally, the others are not with Moscovium being a synthetic element only made in labs.

Group 16: Chalcogens

The Chalcogens have the elements Oxygen, Sulfur, Selenium, Tellurium, and the radioactive element Polonium. Livermorium is a synthetic element that is part of this group. While Oxygen and Phosphorus are abundant in nature, Selenium and Tellurium are not. Polonium is only found in trace amounts due to radioactive decay and Livermorium is made only in labs.

Group 17: Halogens

Halogens consist of Fluorine, Chlorine, Bromine, Iodine, Astatine, and the synthetic element Tennessine. These are non-metals which are poor conductors with low melting and boiling points. The Halogen group is also the only group where at room temperature all three states of matter can be seen in the elements.

Group 18: Noble Gases

Noble Gases are made of Helium, Neon, Argon, Krypton, Xenon, Radon, and the synthetic gas Oganesson. They constitute around 0.96% of the atmosphere. These gases have various uses such as lighting, welding, and space exploration, although they are highly unreactive and colorless in nature.

Kidadl has lots of great name articles to inspire you. If you liked our list of periodic table names then why not learn about these Hungarian last names, or these Indian last names all with history and meanings.

THE STRUCTURE OF AN ATOM

www.google.com/url?q=https%3A%2F%2Fthewordsearch.com%2Fpuzzle%2F8464%2Fatoms%2F&sa=D&sntz=1&usg=AFQjCNHSqdRNl8ALPWg1bjOWJo1eRa0bKw

Atoms are the smallest part of matter that contain protons (+ charge) and neutrons (no charge), inside a nucleus, and electrons (- charge) in electron shells

THE MODEL OF A CARBON ATOM SHOWING ITS ATOMIC STRUCTURE

THE ATOMIC NUMBER AND MASS NUMBER OF AN ATOM

Atomic Number is the number of protons (or the number of electrons)
Mass Number is the sum of protons and neutrons
Atomic number = number of protons = number of electrons
Mass number = number of protons + number of neutrons

Example:

A Carbon atom has an atomic number of 6 and a mass number of 12. How many neutrons are in one atom of carbon?

Mass Number = 12

Atomic Number = 6 = No. of Protons

Number of Electrons = 6

Number of Neutrons = Mass Number - AtomicNumber = 12 - 6

= 6

AN INTERACTIVE ACITVITY FOR YOU!

ELECTRON CONFIGURATION

WHAT IS AN ION?

An ion is formed by the gain or loss of electrons by atoms to become stable

TABLE OF IONS

IONIC COMPOUNDS

CHEMICAL FORMULAS

Ionic Formulae

CHEMICAL EQUATIONS

AN INTERACTIVE BALANCING CHEMICAL EQUATIONS ACTIVITY FOR YOU TO COMPLETE

WHAT IS COMBUSTION?

Combustion is the scientific word for burning. In a combustion reaction, fuel is burned and reacts with oxygen to release energy.

RUSTING

Rusting is the oxidation of iron or iron objects. It takes place in the presence of air and moisture. It is a slow process. Due to rusting, rust is formed on iron objects. It is a red-orange coloured iron oxide that is formed by the oxidation of iron in presence of oxygen and moisture or water.

CHEMICAL EQUATION FOR THE PROCESS OF RUSTING IS GIVEN ABOVE

METALS

NON-METALS

USES OF METALS BASED ON THEIR PROPERTIES

1. Lead (Pb)

Properties: Soft, dense, low melting point, unreactive with water (due to protective oxide layer), and poor electrical conductor.
Uses:
- Car batteries: Its density and ability to be easily cast make it suitable for battery plates.
- Radiation shielding: Its high density makes it effective at absorbing X-rays and gamma rays.
- Roofing/plumbing: Its malleability and resistance to corrosion (due to the oxide layer) made it historically useful for these applications, though its toxicity has led to reduced use.

2. Copper (Cu)

Properties: Excellent electrical and thermal conductivity, malleable, ductile, unreactive with water, and relatively unreactive with dilute acids.
Uses:
- Electrical wiring: Its high electrical conductivity is its most important property for this use.
- Plumbing/pipes: Its resistance to corrosion by water and its malleability make it ideal for water systems.
- Cookware: Its high thermal conductivity allows for even heating.
- Coinage: Its durability and attractive appearance are valued.

3. Zinc (Zn)

Properties: Moderately reactive, forms a protective oxide layer in air, reacts with steam when hot, reacts readily with dilute acids.
Uses:
- Galvanising: Used as a protective coating on steel (e.g., corrugated iron, bolts) to prevent rust. The zinc layer corrodes preferentially to the iron, acting as a sacrificial anode.
- Batteries: Used in dry cell batteries (e.g., alkaline batteries).
- Alloys: A key component in brass (with copper).

4. Aluminium (Al)

Properties: Low density, excellent corrosion resistance (due to strong passive oxide layer), good electrical and thermal conductivity, malleable, ductile.
Uses:
- Aircraft and vehicle construction: Its low density combined with strength (when alloyed) makes it ideal for lightweight structures.
- Food and beverage packaging: Its non-toxicity, corrosion resistance, and malleability make it suitable for cans, foil, and containers.
- Window frames and building materials: Its light weight and resistance to weathering are advantageous.
- Electrical transmission lines: Its good electrical conductivity and low density make it suitable for overhead power lines.

5. Magnesium (Mg)

Properties: Very low density (lightest structural metal), reacts vigorously with oxygen when heated (bright flame), reacts with cold water slowly, reacts very vigorously with acids.
Uses:
- Lightweight alloys: Primarily used in alloys with aluminium to create lightweight and strong materials for aircraft, car parts, and portable electronics.
- Flares and fireworks: Its vigorous reaction with oxygen and production of a bright white light makes it suitable for pyrotechnics.
- Sacrificial anodes: Used to protect other metals (like steel pipelines) from corrosion due to its high reactivity.

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