Y10 Atomic Structure and Chemical Reactions

Ionic bonding occurs between a metal and a non-metal. Metals are located on the left side of the periodic table and non-metals are located on the right side of the periodic table. Due to metals forming cations when theyreact and the non-metals form anions when they react this creates an electrostatic force of attraction between the oppositely charged ions and forms the ionic bond. Non-metal elements are located on the right hand side of the periodic table and they will form covalent bonds with each other to fill their valence shells.

Chemical Change - When a new substance forms during a chemical reaction Physical Change - A change of state or a change of shape and no new substance is formed Physical and chemical changes both cause alterations (some form of change) to the original matter involved. Chemical changes involve the production of a new substance (evidence of a new substance can be fizzing, a colour change or heat/light energy) whereas physical changes do not involve the production of a new substance (they involve changes of state or dissolving). Chemical changes involve the breaking or formation of bonds whereas a physical change is just a change in state/shape. Examples Chemical change: combution, rotting, rusting, digestion Physical change: Melting, shredding, boiling, chopping Signs that a chemical change occured: colour changes,mass changes, temperature changes, a gas may be given off, a sound may be heard

• The chemical elements are arranged in order of increasing atomic number. • The rows (across the table) are called periods and the columns (down the table) are called groups. • Metals are found on the left side of the periodic table and nonmetals found on the right side of the periodic table.

Groups: The Group numbers are at the top of the columns numbered from 1 to 18. All the elements in a group have the same number of electrons in the outer shell (valence shell or orbital) Group 1 = 1 valence electron Group 2 = 2 valence electron Group 13 = 3 valence electrons Group 14 = 4 valence electrons Group 15 = 5 valence electrons Group 16 = 6 valence electrons Group 17 = 7 valence electrons Group 18 = 8 valence electrons Elements in the same group have similar chemical reactions. Periods: Amount of the electron shells The elements found in period 2 will have 2 electron shells. (Li 2.1 ; O 2. 6- two electron shells) Period 3 elements have 3 electron shells. (Na 2.8.1 - three electron shells) Period 4 elements have 4 electron shells. (Ca 2.8.8.2 - four electron shells)

Atoms contain positively charged protons and negatively charged electrons. In an atom, the number of protons and electrons are the same, therefore the charges cancel and there is no overall charge. This makes the atom neutral overall. Neutrons have no charge

Ionic bonding occurs between two oppositely charged ions that are attracted to one another due to electrostatic forces.To form the ions, an (metal) atom will lose valence(s) to form a full valence shell and become stable. The electron(s) lost will be gained by another (non-metal) atom for it to have a full valence shell and become stable. This forms the anion and cation which form the ionic bond and result in an ionic compound. Covalent bonding occurs between two or more non-metal elements. They cannot form a bond by transferring electrons from one to another; instead, they share electrons so that each atom has a full valence shell. This is called a covalent bond.

Silver

Electrical Conductor: Aluminium is a good electrical conductor and is commonly used in power transmission lines. Thermal Conductor: Aluminium is an excellent thermal conductor, making it suitable for heat sinks and cookware. Malleable:** Aluminium is malleable** and can be easily shaped into various forms, making it a versatile material in manufacturing. Lustre: Aluminium has a metallic luster and is often used in decorative applications. Density: Aluminium has a low density, making it lightweight and suitable for applications where weight is a critical factor. Melting Point:** Aluminium has a relatively low melting point**, allowing for energy-efficient processing in manufacturing.

A negatively charged ion

Argon

Smallest complete particle of a matter

Number of protons inside the nucleus of an atom

Gold

Boron

Barrium

Beryllium

Bromine

Carbon

A positively charged ion

• Electrical Conductor: Copper is an excellent electrical conductor, and it is widely used in electrical wiring and electronic components. • Thermal Conductor: Copper is a very good thermal conductor, making it suitable for applications like heat exchangers. • Malleable:** Copper is highly malleable** and can be easily shaped into wires and various forms for different applications. • Lustre: Copper has a reddish-brown color and develops a characteristic patina over time, giving it a distinctive appearance. • Density: Copper has a moderate density, contributing to its strength and versatility in various applications. • Melting Point: Copper has a relatively high melting point, allowing it to withstand the heat generated in electrical applications.

A shared pair of electrons between two or more non-metal elements

Carbonate

Copper

The measure how close the particles in the substance are