Types Of Bonding/ Particles Flashcards
What happens to SOLID particles when the temperature increases and reaches melting point?
heating a solid causes Solid Particles to gain kinetic energy, and vibrate faster.
when temp reaches melting point, the particles use the heat energy to break the forces between them and start melting into a liquid.
Explain each particle (solid, liquid, gas) and what happens in each state
Solid: fixed shape and volume, held together by very strong forces. Arranged and Close to eachother. Vibrate in place.
Liquid: fixed volume, no fixed shape. Randomly arranged but close. Slide over eachother.
Gas: no fixed volume, no fixed shape. Randomly arranged and far apart. Very weak forces between particles causing particles to move quickly in all directions.
What happens to LIQUID particles when temperature increases and reaches boiling point?
When temp increases, particles start to gain kinetic energy and move FASTER and FURTHER APART.
when temp reaches boiling point, particles use all heat energy to break the forces between them and turn into gas.
What type of force holds the oppositely charged ions together in an IONIC BOND?
Electrostatic force
Why do group 1 and group 7 elements react with eachother?
Group 1 elements are alkali metals and all react with the nonmetals in group 7 to form ionic compounds.
Gp 1 elements have one e in their outer shell. Gp 7 have 7 electrons in their outer shells. To get full stable shells of 8 electrons each Gp1 readliy give their outer electron to Gp 7 elements
What happens during the ionic bonding between gp 1 and gp 7?
The gp 1 elements lose one electron to the gp 7 so that gp 1 can form a full outer shell, the gp 7 elements gain an electron to also form a full outer shell.
Gp 1 elements form a positive ion when losing an electron.
Gp 7 elements form a negative ion when gaining an electron.
What happens when atoms lose or gain electrons?
They form ions.
State for each of the below whether they form between metals,nonmetals.
Ionic bonding, Covalent bonding, metallic bonding.
1- ionic bonding form between metals and non metals
2- Covalent bonding form between 2 non metals
3- metallic bonding form between 2 metals
How are metallic bonds different from ionic and covalent bonds?
In metallic bonds, the electrons are free (delocalized) since the electron had very weak attraction between the positive nucleus which caused it to be free. While in ionic bonds the elements share electrons, and in covalent bonds elements transfer electrons.
Why are metals malleable?
Layers of atoms can slide over eachother.
How is metallic bonding good conductors of electricity?
Due to the delocalized electrons that are free to move around and carry the current.
When do ionic compounds conduct electricity, and why?
When ionic compounds are solid, their ions are in a fixed lattice, so can’t flow. However, when molten or aqueous, the ions are free to move and carry charge.
What 3 types of substances can covalent bonds make?
Polymers (chain of molecules strung together)
Giant covalent structures
Simple molecular substances
Give 3 examples of giant covalent structures.
Silicon dioxide, diamond, graphite
Describe the bonding in simple molecular substances.
There are strong covalent bonds between the atoms of each molecule, but weak intermolecular forces between the different molecules.
Why do simple molecular substances have low melting and boiling points?
the intermolecular forces between the molecules are weak, so only require a small amount of energy to break. Which means they can break in low temperatures.
Describe the structure and bonding of diamond.
Giant covalent lattice structure.
Each carbon is covalently bonded to 4 other carbon atoms, forming a repeating lattice.
Can graphite conduct electricity? Explain why.
Graphite is a good conductor of electricity. Because graphite contains delocalized electrons which are free to move around and carry charge.
State the definition of an alloy and how is it stronger than a pure metal-
An alloy is a mixture of a metal and another element; steel could be an alloy since it contains iron and carbon
The different elements have different-sized atoms. (Carbon is a different size and iron is a different size)
This distorts the regular layered structure.
Meaning the layers can’t slide over one another anymore.
This makes alloys stronger
State the definition of a metal and how it is weaker than an alloy-
A substance with high electrical conductivity, which lose electrons to form cations.(positive ions)
Metals contain atoms of the same size
Atoms can slide over eachother
Metal is soft, making it weaker.
State the definition of nano particles, it’s key features and it’s uses-
Nano particles are very small particles.
Key features: large surface area to volume ratio (as things get smaller the volume decreases rapidly than their surface area)
Uses- ~To deliver drugs around the body
~Nanoparticles can be infused into surgical masks and wounds.
~ nanoparticles can be used in electrical circuits, since some of them can conduct electricity, so they can create tiny computer chips.
Issues with nanoparticles-
Nanoparticles are relatively new, not much research has been done. Effects on our bodies aren’t fully understood.
State the physical properties of diamond-
Diamond does not conduct electricity-
There are no delocalized electrons that are free to carry a charge/current.
Diamond has a high melting point-
Giant covalent structure
Strong covalent bonds between these carbon atoms which requires high energy to break those bonds leading to HMP.
Extremely hard and dense-
Each carbon atom bonds with 4 other carbon atoms, forming a repeating lattice, leading to a hard structure.
State the properties of graphite-
Graphite can conduct electricity-
Each carbon atom forms 3 strong covalent bonds with 3 other carbon atoms, leaving one free electron per carbon atom.
This delocalized is able to move between the layers to carry a charge.
Graphite has a high melting point-
Giant covalent structure
Strong covalent bonds between the carbon atoms
Graphite is soft and slippery-
Although there is strong covalent bonds between the carbon atoms, there are weak intermolecular forces between the layers, and there are no covalent bonds between the layers, causing the layers to be able to slide over eachother, leading to graphite being soft and slippery.
Compare between metals and alloys-
Metals-
Contains only one element
Contain Atoms of the same size
Atoms slide over eachother
Soft, weaker than alloys.
Alloys-
Contains a mixture of elements
Contain atoms of different sizes
Not able to slide over eachother easily
Which makes alloys harder and stronger than a pure metal
Explain in terms of particles why rate of reaction increases by temperature- 4 marker
Particles gain higher kinetic energy.
Particles move faster.
Leading to more collisions between particles.
More particles reaching activation energy.
How will increasing the pressure increase the rate of reaction?
Increasing the pressure of reacting gases will increase the frequency of collisions which increases the overall rate or reaction
How do you test for double bonds?
Alkenes will react with bromine water and turn from an orange brown to a colourless solution in the presence of double bonds.
Since diatomic elements are two atoms that are bonded in a molecule, that means it exists as I2, H2, O2,Cl2: How come in compounds such as NaCl there’s only one Cl atom?
Since diatomic elements only need to pair up when they’re in their own. So if they’re found in compounds: they don’t need to have two atoms. Only when their by themselves they need to be in pairs,
What is a covalent bond?
Shared pairs of electrons
What are the difference between a monatomic and diatomic molecules?
Monatomic: one molecule which contains only one atom
Diatomic: two atoms that are covalently bonded in a molecule
Why do ionic compounds have high melting/boiling points? 2 marks
Because of the large amounts of energy needed to break the strong bonds.
Do ionic compounds conduct electricity when molten/dissolved?
Yes because the ions are free to move around to carry the CURRENT.
What is the structure of fullerenes?
Based on hexagonal rings of carbon atoms
What happens when you increase the concentration/ or surface area of reactants?
Increasing the concentration/surface area of reactants in solutions causes the frequency of collisions to increase, leading to an increase in the ROR
What is the process when solid turns into a gas, etc-
S into G- sublimation
G into S- deposition
Solid to liquid- melting
L to S - freezing
L to G- evaporation
G to L- condensation
What is deposition? Sublimation? Melting? Freezing?
Deposition- change of state from a gaseous state to a solid state without becoming a liquid in the process.
Sublimation- change in state from a solid state into a gaseous state.
Melting- change from a solid state into a liquid state.
Freezing- change from a liquid state into a solid state.
How many electrons are shared in a single bond, a double bond and a triple bond-
Single bond- two atoms share one electron
Double bond- two atoms share 2 pairs (4) of electrons ( oxygen for example- each oxygen atom gains 2 electrons, so the two atoms gain 4 electrons in total)
Triple bond- two atoms share 3 pairs (6)of electrons
Why do simple molecules have low MP such as water?
Since simple molecules are small and they have weak intermolecular forces between their molecules.
Explain, in terms of bonding why pure water does not conduct electricity-
Because pure water is covalent, so the ions are not free to move to carry a charge.
Why is graphite used as a lubricant?
Graphite has weak intermolecular forces between the layers, making the layers able to slide over eachother, and so graphite is soft and slippery which is the properties of lubricants
What is the mass of the sub- atomic particles?
Neutron- 1
Proton - 1
Electron- very small, or 1/1840
What are molecules?
Atoms of the same element
CH4 and CH4 - these both are atoms that are not bonded, how do u write them down?
2C H4, since they’re not bonded so we write the 2 outside
(C2H8, C2H4) wrong
If Fe atoms are magnetic when bonded, will they have the same properties when they’re single?
Nope, they will share different properties when they’re alone.
