Atoms and reactions
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- Created by: Hannah
- Created on: 19-04-13 12:28
What is the relative mass, charge and location of protons, neutrons and electrons?
P: M=1 C=+1 N: M=1 C=0 E: M=1/2000 C=-1
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How do you work out number of neutrons in an element?
Take away the mass number(top number) away from the atomic number(bottom number)
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In an isotope what part of the element changes?
Neutron number
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In an ion what part of the element changes?
Proton and electron number. Negative ions have more electrons than protons. Positive ions have less electrons than protons.
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How many electrons and protons will Cl- have?
18 electrons, 17 protons
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How many electrons and protons will Mg2+ have?
10 electrons, 12 protons
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Define isotope
Atoms of the same element with a different number of nuetrons
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Define relative atomic mass (RAM) Ar
The weighted average mass of an atom of an element on a scale where an atom of Carbon-12 is 12.
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Define relative isotopic mass
The mass of an isotope of an element on a scale where an atom of Carbon-12 is 12
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Define relative molecular mass (or relative formula mass) Mr
The average mass of a molecule or formula unit on a scale where an atom of Carbon-12 is 12
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How can you work out the Ar from isotopic abundances?
Multiply each relative isotopic mass by its % relative isotopic abundance, add the results up. Then divide by 100.
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What is the equation for working out moles from concentration?
No. of moles= conc. x vol (in cm3) / 1000
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What is the equation for working out the number of moles from a gas volume in cm3?
No. of moles= volume in cm3/ 24000
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What is the equation for working out the number of moles from a gas volume in dm3?
No. of moles= volume in dm3/ 24
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What ions do acids release in aqueous solution? What is this called?
H+. Proton donors?
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What are proton acceptors?
Bases. They remove H+ ions from an aqeous solution
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Define the term salt.
When the hydrogen ions in acids are replaced by metal ions or ammonium ions (NH4+)
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What is the equation for a metal oxide reacting with acid?
Metal Oxide + Acid - Salt + Water
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What is the equation for a metal hydroxide reacting with acid?
Metal Hydroxide + Acid - Salt + Water
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What is the equation for reacting ammonia with acid?
Ammonia + Acid - Ammonium salt
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What is the equation for reacting a metal with an acid?
Metal + Acid - Metal salt + Hydrogen
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What is the equation for reacting a metal carbonate with an acid?
Metal carbonate + Acid - Metal salt + Carbon dioxide + Water
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Define an anhydrous salt.
A salt that doesnt contain water of crystalisation.
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Define a hydrated salt.
A salt that does contain water of crystalisation
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What indicator turns yellow to red when adding acid to alkali?
Methyl orange
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What indicator turns red to colourless when adding acid to alkali?
Phenolphthalein
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Define oxidation
The loss of electrons
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Define reduction
The gain of electrons
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Define oxidising agent
Accepts electrons and gets reduced
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Define reducing agent
Donates electrons and gets oxidised
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What is the oxidation of an uncombined element e.g. Ca
0
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What is the oxidation of elements bonded to identical atoms e.g O2
0
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What is a dispropotiation reaction?
Where the same element in different compounds gets both oxidised and reduced
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What is the maximum electrons that can be in the S sub-shell
2
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What is the maximum electrons that can be in the P sub-shell
6
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What is the maximum electrons that can be in the D sub-shell
10
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What is the maximum electrons that can be in the F sub-shell
14
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What is the maximum electrons that can be in the 3rd shell
3s, 3p, 3d, 18
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Define an orbital
The space in which an electron moves in
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Do orbitals with the same sub-shell have the same energy?
Yes
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Define spin-pairing
When electrons in the orbitals have to spin in opposite directions
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What shape are S orbitals
Spherical
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What shape are P orbitals
Dumbbel shapes, there are 3 P orbitals and they are at right angles to eachother
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If an ion is X2+ do they have a lager or smaller Electronic Configuration?
Smaller
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Define 1st ionisation energy
The first ionisation energy is the energy needed to remove 1 electron from each atom in 1 mole of gasous atoms to form1 mole of gasous 1+ atoms
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What is the equation for the 1st ionisation of Oxygen?
O(g) - O+ (g) + e-
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What are the state symbols for ionisation equations?
ALWAYS (g)
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How does nuclear charge affect ionisation energy?
The more neutrons there are in the nucleus, the more positively charged the nucleus is and the stronger the attraction for electrons
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How does distance from the nucleus affect ionisation energy?
Attraction falls rapidly with distance. An electron close to the nucleus will be much more strongly attracted than one further away
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How does sheilding affect ionisation energy?
As the number of electrons between the outer electrons and the nucleus increases, the outer electrons feel less attraction towards nuclear charge
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What does high ionisation energy mean?
There's a high attraction between the electron and the nucleus
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Does sheilding affect a period?
No, as all the electrons are in the same shell
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What is the trend for ionisation energies?
Within each shell successive ionisation energies increase because electrons are being removed from an increasing positive ion (more attraction from the nucleus to the electrons)
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How does the ionisation energy change when you go into a new shell?
There is a big jump as you are removing electrons that are getting closer to the nucleus
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Define ionic bonding
Is the bond formed by electrostatic attraction between two negatively charged ions
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When do ionic compounds conduct electricity?
When they're molten. But NOT when they're solid. This is because in a solid the ions arent free to move (then carry charge)
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Why do ionic compounds have high boiling points?
The giant ionic lattices are held together by strong electrostatic forces, take a lot of energy to overcome these forces
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Why do ionic compounds dissolve in water?
Water molecules are polar, part of the molecule has a small negative charge and the other bits have small positive charges. Water molecules pull ions away from the lattice to dissolve it
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Define covalent bonding
A shared pair of electrons
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What are diamond and graphite?
Giant convalent lattices
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Define giant covalent lattice
Huge networks of covalently bonded atoms (sometimes called macromollecular structures)
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Why can carbon form this type of structure?
Because they can each form four strong covalent bonds
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State some properties of diamond (due to covalent bonds)
Has a high melting point (over 3800K) , is very hard- used in cutting tools, its a good thermal conductor due to vibrations being able to travel easily, it cant conduct electricity- all outer electrons are held in bonds, it wont dissolve
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State some properites of graphite (due to covalent bonds)
Weak bonds between layers, graphite is easily broken, so is slippery and used as lubricants, can conduct eletricity due to delocalised electrons, layers are quite far apart, so is leighweight and used in sports equipement, high melting point
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What are the sheets in graphite bonded by?
Van der Waals
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State properties of giant metallic lattice structures
Delocalised electrons leave a positive metal ion, the positive metal ions are attracted to the delocalised electrons, this forms the lattice and metallic bonding
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How does the number of delocalised electrons affect the melting point?
The more delocalised electrons there are, the stronger the bonding will be and the higher the melting point
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What makes it malleable and ductile?
As there are no bonds that actually hold specific ions together, they can slide past eachother and be pulled, hammered into sheets (malleable) and drawn into wires (ductile)
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What makes them good thermal conductors?
The delocalised electrons can pass on kinetic energy to eachother
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Why do they conduct electricity?
Delocalised electrons can pass on a current
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Why are they insoluble?
All solid metals are insolube because of the strength of the metallic bonds, however liquid metals can
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Other cards in this set
Card 2
Front
How do you work out number of neutrons in an element?
Back
Take away the mass number(top number) away from the atomic number(bottom number)
Card 3
Front
In an isotope what part of the element changes?
Back
Card 4
Front
In an ion what part of the element changes?
Back
Card 5
Front
How many electrons and protons will Cl- have?
Back
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