Types of Chemical bonds - Q2

outer electronic shells

Most elements are not stable in terms of their?

The three types of Chemical bonds

Covalent, Ionic, and Metallic bonds

In order to achievel stability by producing a stable compound.

Why do some elements need to bond together?

Ionic Bonds

It is when a metal and a non-metal react together, the metal atom loses electrons to form a positively charged ion and the non-metal gains these electrons to form a negatively charged ion just for them to bond.

Ionic Bonds.

The oppositely charged ions between non metals and metals are strongly attracted to one another by electrostatic forces. this attraction is known as?

Ions

These are charged particles and can be either be single atoms or groups of atoms such as compounds.

Ionic bonds have _____ high melting points and boiling points due to the strong points of attraction between the ions.

Stable

A particle with a full outer shell is considered what?

A full outer shell.

Some particles will either lose or gain electrons in order to achieve what?

conduct electricity

Solid ionic compounds can’t _________

dissolve easily

Ionic compounds _______ in water, seprating the ions which allows it to conduct electricity as they are free to move.

conduct electricity

Only both dissolved or melted ionic compounds can what?

Giant ionic lattice

What is the structure of ionic compounds?

Ionic bonds

These bonds form a closely packed lattices arrangement while having strong electrostatic forces of attraction in all directions

Mettalic bonds

These bonds results from the metal atom’s outer shell electrons being delocalised (free to move around).

Mettalic bonds

The bond originate from the strong forces of electrostatic attraction between positive metal ions and the shared negative electrons.

Metals

what are solid at room temperature - the electrostatic forces between these ions and delocalised electrons require alot of energy to be broken.

Metals

These are good conductors of heat and eletricity - This is due to the delocalised electrons’ ability to carry current and thermal energy through the whole structure.

malleable

Most metals have this property where the layers of atoms within a metal can slide over each other, this means that metals can be bent, hammered, or rolled into flat sheets.

Alloys

These can increase the hardness of metals - different metals have different sized atoms.

Alloys

Mixing a metal with another results in those layers becoming distorted, making it difficult for the layers to slide past each other. Thus, these are harder than pure metals.

Covalent bonds

It is when non-metal atoms bond together by sharing pairs of electrons.

electrostatic forces

The positively charged nuclei of the covalent bonded atoms are attracted to the negatively charged shared electrons by what forces, making these bonds strong?

high

Covalent bonds have very ____ melting and boiling points as lots of energy is needed to break the covalent bonds.

Covalent bonds don’t conduct electricity.

Covalent bonds don’t contain charged particles, this means that? pick the correct statement?

Covalent bonds

• Diamond

• Graphite

• Silicon Dioxide.

are main examples of what type of bonds?

graphite and graphene

Each carbon atom in this substance forms three covalent bonds to create layers of hexagons.

Graphene and graphite

These compounds are able to conduct electricity and heat

diamond

ach carbon atoms forms four covalent bonds in a very rigid giant covalent structure, making this substance  really hard.

Silicon dioxide.

Also known as silica, each grain of sand is one giant structure of silicon and oxygen.. what compound it this?