Paper 1 Flashcards
What is an Ion?
-An atom that either loses/gain electrons
-To from a charged particle
Give the Relative Mass & Relative charge of Subatomic Particles
PROTONS
RM - 1
RC - +1
NEUTRON
RM - 1
RC - 0
ELECTRON
RM - 0.0005
RC - -1
What is the Atomic Radius of an Atom?
10(-10)m
1.What is the Mass No.
2. What is the Atomic No.
3.How do you find the No. of neutrons
- No. Of Protons + Neutrons
- Proton No. (=Electrons No.)
- Mass No. - Atomic No.
Give the History of the Atom
-Dalton - Solid spheres, couldn’t be broken down, different for different elements
-Thompson - discovered the charge & mass prove smaller particles, (-) electrons. (PPM)
-Rutherford - gold foil exp. (alpha particles), PPM, some where deflected backwards (not fully positive atom). Nuclear Model, (+) nucleus, electrons surround nucleus. Nucleus deflected alpha particles
-Bohr - ‘cloud’ electrons would attract nucleus and collapse atom. Electrons contained in shells.
What is an Isotope?
Different forms of the same element, which have the same number of protons but a different number of neutrons.
Isotopes have the same (1)________ _____ but a different (2) ________ _____.
- Atomic Number
- Mass Number
What is Electrolysis?
The process of using electricity to separate the elements in insoluble ionic compounds.
What is an Electolyte?
A liquid/solution that contains an ionic compound (ions are free to move)
What are Electrodes?
Electrical conductors in Electrolysis
Why must electrolytes be molten/liquid?
So the ions are free to move
If a metal oxide is less reactive than carbon, then they are split by the Reduction of Carbon. Why do industries prefer this?
Because it’s cheaper than electrolysis.
The Anode is (1)_________ and (2)_____________ ions.
The Cathode is (3)_________ and (4)___________ ions.
- Positive
- Oxidises
- Negative
- Reduces
The Negative Cathode attracts the (1)_________ ion from the compound, and the positive anode attracts the (2)_________ ions.
- Metal
2.Negative
What ions would you find in the water of an electrolyte?
Hydrogen and Hydroxide ions
What is a Covalent Bond?
Strong bonds that are formed when a pair of electrons are shared between atoms.
- Give the three examples of Simple Molecular Substances?
- What do they all have in common?
- Any from: Hydrogen, Hydrogen Chloride, Water, Methane, Oxygen, Carbon Dioxide.
- All made by Covalent Bonds
Substances containing covalent bonds normally have what?
Simple Molecular Structures (e.g. H2O and CO2)
Covalent Bonds are very (1)________, however they have weak (2) _____________ _______.
- Strong
- Intermolecular Forces
Properties of Covalent Bonds
• Melting/Boiling Points are low (breaking the intermolecular force, not bond)
• (most) substances are gases/liquids at room temp.
• Bigger Molecules have bigger M.p/B.P because the strength of intermolecular forces increases.
• Don’t conduct electricity (not charged, no free electrons/ions).
What is Metallic Bonding, and what does it involve?
Bonding between Metals only.
It involves the electrons on the outer shell being delocalised, there are strong forces of electrostatic attraction between the +ions and -ions. These forces hold the atoms in a regular structure.
What are the Properties of Metals/Metallic Bonding?
• High M.p/B.p (strong electrostatic forces between ions & delocalised electrons are strong, so more energy is needed).
• Shiny Solids (at room temp).
• Not soluble in Water
• More dense than non-metals (ions closely packed)
• Malleable
• Good Conductors of Electricity
What are Fullerenes and what is their bonding?
Fullerenes are molecules made up of carbon atoms, arranged into rings and structured like a tube or hollow sphere.
They are made from Covalent bonding.
- Why are fullerenes used to deliver drugs around the body?
- Why are Fullerenes good industrial catalysts?
- The fullerene structure is hollow so it can ‘cage’ other molecules (the drug). This then allows it to deliver a drug directly to the cell.
- They have a huge surface area, which allow other individual catalysts to be attached to them.
Give the two main Fullerenes.
Nanotubes and Buckminsterfullerene
Explain what a carbon Nanotube is and its properties
A carbon nanotube is a type of fullerene, structured like a hollow tube and is made of cylinders of graphene (causes it to conduct electricity)
PROPERTIES
• conducts electricity
• high tensile strength (don’t break when stretched) - used to strengthen materials without adding weight (e.g sports equipment).
Explain what Buckminsterfullerene is and give its molecular formula
Buckminsterfullerene is a hollow sphere made up of carbon hexagons/rings; it’s a stable molecule that forms soft brown/black crystals and has a molecular formula of C60.
What is a Polymer and how is it formed?
Polymers are molecules of long chains, made of covalently bonded carbon atoms. They are formed when smaller molecules called monomers join together.
Give a famous example of a Polymer
Poly(ethene)
Why doesn’t the mass in a closed system change?
Because there is no way the products can evaporate/escape, therefore the mass will remain the same. (Also because no atoms are created or destroyed).
What does it mean is the mass increasing during a chemical reaction?
Because one of the reactants will (probably) be a gas.
The gas is in the air, but not in the reaction vessel (can’t measure its mass). During the reactions, the gas reactants with the reactants to form the product, so the mass of the reaction vessel increases
What does it mean if the mass decreases during a chemical reaction?
Before the reaction, all the reactants are in the reaction vessel. If the vessel isn’t enclosed then the gas can escape (evaporation), therefore the total mass inside the reaction vessel decreases.
