C2 Flashcards
Atom
Smallest possible piece on an element. Has a radius of 0.1nm
Proton
A positively charged particle found in the nucleus. Has a relative mass of 1
Neutron
A neutral particle found in the nucleus has a relative mass of 1
Electron
A negatively charged particle found in energy levels (shells) around the nucleus. Has a relative mass of 1/2000
Ionic Bond
Occurs between a metal and non metal element, where the metal atom loses electrons to a non metal atom to form ions
Electrostatic force of attraction
An attraction that occurs between positive and negative changes
Giant ionic lattice
Made up of billions of oppositely charged ions that are held together by strong forces of attraction
Molten
heating a solid and turning it into a liquid
Covalent bonding
Occurs between two or more non-metal atoms where electrons are shared
Giant Covalent substance
Billions of atoms all joined up together by covalent bonds
Intermolecular force
Weak attractive forces between molecules. When a simple molecular substance melts or boils. It is the intermolecular forces that are broken (not the covalent bonds in each molecule)
Polymer
Millions of small molecules joined together in a chain to form a large molecule
Graphene
One layer of graphite
Fullerene
A substance made of carbon atoms arranged in a cage
Nanotube
Cylindrical fullerenes that are used in electronics, nanotechnology and materials
Metallic bond
An electrostatic attraction between positively charged ions and delocalized electrons
Malleable
Can be bent or shaped without breaking
If an atom gains an electron what does it become
A negative ion (Anion)
If an atom loses an atom what does it become
A positive ion (Cation)
What is the charge on elements from group 1 and 2
Group 1:+1
Group2:+2
What is the charge on elements from group 6 and 7
Group 6: -2
group 7: -1
Explain why ionic compounds have high melting points
Giant ionic lattice held by strong electrostatic force of attractions between the positive and negative ions
Explain why ionic compounds do not conduct electricity when solid
The ions are not free to move and carry charge
How many electrons are in 1 and 2 covalent bonds
1 Covalent bond = 1 pair of electrons
2 Covalent bond = 2 pair of electrons
Explain why diamond and silicon dioxide have high melting points
They are both giant covalent structures which contain a lot of covalent bonds between the atoms
Why is diamond and silicon dioxide hard
Strong covalent bonds between the atoms
What type of substance is water and methane?
Simple molecules
Explain why small molecules have a low melting point
The intermolecular forces are easy to break
Explain why most Covalent substances do not conduct electricity
No electrons that carry charge or are free moving
Explain why metals have high melting and boiling points
Strong electrostatic attractions between the positive metal ions and delocalized electrons. Lots of thermal energy is needed to break them
Explain why metals are good conductors of both heat and electricity
Delocalized electrons can carry charge
