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69 Cards in this Set
- Front
- Back
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What is the name of the energy required to move an electron from a ground state to n=∞? |
First ionization energy |
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What transitions from energy levels correspond to different light transmissions in hydrogen? |
3rd level is infra-red 2nd level is visible light 1st level is UV light |
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What happens at the top of energy spectrums? |
Convergence, where energy levels converge. |
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What is Shrodigners theory? |
A wave equation to describe electrons behaviour in multi-electron systems. |
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What is the solution of Shrodigners theory? |
The solution gives us atomic orbitals, which is a region where there is a 90% probability that the electron will be found. |
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What are the electron sub shells? |
There are four sub shells, s, p, d and f. |
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What are orbitals? |
Orbitals are found within energy sub shells, each orbital can only hold 2 electrons. |
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Why can two electrons occupy the same orbital? |
Because they spin in different directions. |
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How many electrons can each main level hold? |
2n^2 |
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Draw the AufBun diagram. |
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Write the shorthand electron configuration for Vanadium. |
[Ar]1s^2 2s^2 3s^2 3p^6 4s^2 3d^3 |
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Draw a box and arrow diagram for Oxygen |
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What is Planck's equation? Define. |
E=hv E energy h constant (6.63x10^-34) v frequency |
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What are some patterns in ionization energy of singular elements? |
-Ionization energy increases as more electrons are removed, because remaining electrons are closer to the positively charged nucleus. -There are large increases between energy shells -Small jumps between energy subshells |
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What are some ionization energy patterns of elements as a whole? |
-Noble gases have a much higher energy level -However, this decreaes down the group -Atoms in the first group are much less stable, and therefore have a much lower first ionization energy. -When there is more than one electron in an orbital, that electron is easier to remove as a result of repulsion. |
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Who invented the periodic table? |
Mendeleev |
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What are the four group names? |
1: Alkali metals 2: Alkaline earth metals 17: Halogens 18: Noble gases |
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What are three properties of alkali metals? |
-React with water to from an alkali solution of the metal hydroxide and hydrogen gas -React by losing outer electron to form ion -Good reducing agents because they can readily lose electrons. |
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What are three properties of alkaline earth metals? |
-Abundant metals in the earth -Not as reactive as alkali metals -Higher density and melting point than alkali metals |
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What are four characteristics of transition metals? |
-Variable valency and oxidation state -Form coloured compounds -Form complex ions -Catalytic behaviour |
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What are three characteristics of halogens? |
-React by gaining one electron to form hallide ion -Good oxidising agents -Opposite to alkali metals |
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What are seven periodic trends? |
-Valence -Atomic radii -Ionic radii -Electronegativity -Electron affinity -Ionization energy -Melting point |
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What are the three factors that generally explain periodic trends? |
-Nuclear charge -Number of shells -Amount of shielding |
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What does electron attraction depend on? and what is it called |
-Protons in nucleus -How far the electron is from the nucleus -Amount of core electrons Called effective nuclear charge |
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How do you work out effective nuclear charge? |
Nuclear charge - core electrons = approximate nuclear charge |
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What are effective nuclear charge trends? |
-Same down a group due to increase in core electrons. increases by one across a group. |
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What is atomic radii and how is it defined? |
-Atomic radii is the distance from the nucleus to the outermost electrons -Defined as half the distance between the nucleus and two bonded electrons of the same element |
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Explain the trends of atomic radii. |
1. Increases down the group Because increasing number of core electrons shield the nucleus. Known as effective nuclear charge. 2. Decreases across a period Because protons in nucleus increase, so does electron attraction. |
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Explain the trends of ionic radii. |
1. For both anions and cations, radii increases down the group. Outer electrons are in higher energy levels and further away from the group 2. For both cations and anions, ionic radii decreases across a group Along the period, ions are attracted to increasing positive charge. Cations become smaller than original atom, anions become larger than original atom then decrease in size |
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Explain the trends in first ionization energy. |
1. Decreases down a group Electrons are in higher energy levels further away from the pull of the nucleus and therefore easier to remove. Coulomb Force is reduced 2. Increases along a period Increasing nuclear charge exerts a greater pull on the electrons. Energy must be put in to remove electron, therefore is endothermic. |
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What is electron affinity? |
-The energy change when one mole of electrons is added to one mole of gaseous atoms to from one mole of gaseous ions. |
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Name the trends in electron afffinity. |
1. Decrease down the group Increasing number of core elctrons means the outer electrons are further away from the nucleus, and have a lesser attraction. 2. Increases across a period Increasing effective nuclear charge means that electrons are more attracted to the nucleus. |
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What is electronegativity? |
-A relative measure of the attraction that an atom has for a shared pair of electrons when they are constantly bonded, tells us which the shared electrons spend more time around. |
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Explain the trends in electronegativity. |
1. Decreases down a group Larger size produced by extra energy levels means decreased attraction, electronegativity. 2. Increases across a period (noble gases excluded) AS nuclear charge increases, atomic radius is decreasing, therefore attractive forces that the nucleus can exert on other electrons increases. |
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What does melting point depend on? |
-Structure of the elements -Type of attractive forces holding atoms together |
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Name the different melting point trends |
-Elements on the left have metallic bonding, and are therefore stronger -Melting point decreases down groups 1 and 2 because atoms become larger, reducing strength of attraction. -Silicone is in the middle and has macromolecular structure with very strong bonds -Group 5,6,7 have weak attraction, therefore low melting point, due to weak bonds -Noble gases exist as individual atoms, and have weak attractive forces -Group 17 has increasing melting point because Van Der Waals attractive forces between diatomic molecules increase down the group |
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What are the reactivity trends? |
-Alkali metals increase down the group -Halogens decrease down the group (because of electronegativity) |
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What happens if an alkali is mixed with water? |
An alkaline will be formed |
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In halogen displacement between halogens, hallides, and alkali's, how do you know which halogen will be displaced? |
-Whichever halogen is highest on the periodic table will displace the other |
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What structure do each of the group 3 element oxides have? Do they conduct electricity? Are they basic or acidic? |
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What is ampoheric? |
Can act as acid and base. |
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How do we work out acid base character? |
By mixing them with water. |
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Give an example of an acid base reaction. |
Na2O + H20 --> 2NaOH (base) |
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Name the relative mass and relative charge of the sub-atomic particles. |
Relative mass: Proton 1 - electron .005 - neutron 1 Relative charge: Proton +1 - electron -1 - neutron 0 |
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What is an isotope? How do their properties differ? |
Atoms of the same element with differing amounts of neutrons. They have the same chemical properties, but different physical properties. |
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If electrons leave or come, what do they create? |
ions. positive are called cations, negative are called anions. |
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What instrument is used to measure the mass of individual atoms? What are the problems? Therefore, what do we usually use. |
A mass spectrometer, giving us a mass spectrum with mass on the x and percentage abundance on the y. However this gives very complicated values, so we usually use relative atomic mass. |
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What is relative atomic mass? |
The mass of all the elements in relation to carbon 12 |
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What are the low energy waves and what are the high energy waves? |
Low energy is radio waves, high energy is gamma rays. Radio ways also have a large frequency. |
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What is c=V λ |
velocity of light = frequency x wavelength . velocity of light is a constant, so we can work out the other variables. |
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What is a spectrometer and how is it used? |
A spectrometer will pass white light through atoms of an element an create an emission spectrum. We can then produce the absorption spectrum, giving us information about the configuration of the atoms. |
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What is E=hv |
Energy = plancks constant x frequency |
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What is plancks constant? |
6.63 x10^-34 |
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Draw an s-orbital |
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Draw a p-orbital |
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How many electrons can each main level hold? |
2n^2 |
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What are the three d-block rules? |
1. It is written in lower energy to 4s block 2. Chromium has configuration Ar 3d^5 4s^1 3. Copper has configuration Ar 3d^10 4s^1 |
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What is a mole? |
6.02 x10^23 particles of a substance. |
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What is the number of moles mass molar mass equation? |
n = m/M answer will be given in unit gmol^-1 |
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How do we work out number of particles from mole? |
no. of moles = number of particles/6.02 x 10^23 |
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What is an empirical formula? |
The simplest ratio of the elements in a compound. |
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How do you find molecular formula from empirical formula? |
mass of empirical formula/real mass |
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How do we work out percentage error? |
experimental value - theoretical value/theoretical value |
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What is a limiting reactant? |
The reactant that you do not have enough of, which will then determine how much product is formed. |
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How do we work out percentage yield> |
experimental yield/theoretical yield x 100 |
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What is a solution and its components? |
Solution, something dissolved in something. Solvent: liquid used to dissolve solute Solute: the soild that is dissolved |
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What is the concentration formula including units? |
c = n/v c concentration n number of moles (solute) v volume dm^3 (litres) (solvent) |
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What are the three units of measurement in concentrations? |
dm^3 - equal to 1L gdm^-3 mass of solute per dm^3 of solvent ppm parts per million mass of solute x 10^6/total mass of solution |
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How do we work out dilutions? |
n will stay the same so we can assume that for the solutions cv=cv |
