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Che144 > Week 1 Matter > Flashcards

Week 1 Matter Flashcards

1
Q

What is a Quantum?

A

The smallest amount of energy that ca be emitted/absorbed as electroradition.

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2
Q

What is Planck’s constant?

A

6.626 X 10^-34 (Joules seconds)

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3
Q

What is Planck’s theory?

A

Matter is allowed to emit/absorb energy only in whole number multiples.

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4
Q

What are the 2 rules of Bohr’s model.

A
  1. Electrons exist only in certain discrete energy levels, which are described by quantum numbers.
  2. Energy is involved in moving an electron from one level to another.
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5
Q

What is the orbitals probability density?

A

The orbitals probability density describes a specific distribution of electron density in space.

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6
Q

What is the principal quantum number (n)

A

This number describes the size of the orbital, with 1 being the smallest. An increase in (n) means the orbital electron is less tightly bound to the nucleus.

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7
Q

What is the angular momentum quantum number (i)

A

Defines the shape of the orbital, with values from 0 to n -1. E.G n=3, i=0,1,2.

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8
Q

What is the magnetic quantum number (m)

A

Describes the orientation of the orbital in space via integral values between -1,0,1

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9
Q

What is the electron shell

A

A collection of orbitals with the same value of (n) E.G n=3 is the third shell

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10
Q

What is a subshell?

A

A set of orbitals that have the same (n) and (i) values.

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11
Q

What are degenerate orbitals?

A

Orbitals wit the same energy.

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12
Q

What is the Pauli exclusion principle?

A

No two electrons can have he same set of four quantum numbers (n,i,Mi, and Ms) in the same atom.

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13
Q

Wha is the electron configuration?

A

The way in which the electrons are distributed among the various orbitals of an atom.

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14
Q

What is the Aufbau principle?

A

Oribitals are filled in order of increasing energy, with no more than 2 electrons per orbital.

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15
Q

What is hund’s rule?

A

For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximised.

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16
Q

What are the Lanthanide elements?

A

The 14 elements corresponding to the filling of the 4f orbitals (rare earth elements)

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17
Q

What are Actinide elements?

A

Elements in the final row of the periodic table that start to fill the 7s orbital (Radioactive).

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18
Q

What is the Actual nuclear charge (Z)

A

The number of protons in the nucleus.

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19
Q

What is the Effective nuclear charge?

A

The charge that valence electrons see.

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20
Q

What is the Bonding atomic radius?

A

Half the distance between 2 identical atoms nuclei that are chemically bonded to each other.

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21
Q

What is the Isoelectronic series?

A

A group of ions all containing the sae number of electrons.

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22
Q

What is Ionisation energy?

A

The smallest amount of energy required to remove an electron from the ground state of the isolated gaseous atom or ion
(Lose of electron)

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23
Q

What is Electron affinity?

A

The energy change that occurs when an electron is added to a gaseous atom or ion
(Gain of electron)

24
Q

What is an ionic bond?

A

Electrostatic forces between ions of opposite charge.

25
Q

What is a Covalent bond?

A

The sharing of electrons between 2 atoms.

26
Q

What is metallic bonds?

A

Each atom in a metal is bonded to several neighbouring atoms.

27
Q

What is the octet rule?

A

Atoms tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons.

28
Q

What are non-polar covalent bonds

A

Bonds where electrons are shared equally between two atoms

29
Q

What are polar covalent bonds

A

A bond where one of the atoms exert a greater attraction for the bonding electrons than the other atom

30
Q

What are resonance structures

A

A Lewis structure that has more than one correct way of displaying it

31
Q

What is a dipole moment

A

A quantitative measure of the amount of charge separation in the molecule

32
Q

What are addition reactions

A

The most characteristic reactions of alkenes and alkynes in which a reactant is added across the two carbon atoms that form the multiple bond

33
Q

What are Electrophiles

A

Molecules that accept a pair of electrons in a chemical reaction

34
Q

What are nucleophiles

A

Species that donates a pair of electrons in a chemical reaction

35
Q

What is a stereoselective reaction?

A

A reaction in which the product has one particular geometry in preference over another

36
Q

What does a Bold wedge indicate?`

A

Indicates that the direction of the bond is extending towards the viewer off the plane of the paper

37
Q

What does a dashed wedge indicate?

A

Indicates the direction of the bond is directed into the paper away from the viewer

38
Q

What is a Chiral

A

All molecules that contain a single carbon atom bearing four different groups

39
Q

What is a Enantiomer?

A

Two molecules that are non-superimposable mirror images

Always have a chiral centre

40
Q

What is a Achiral

A

Molecules that are superimposable.

Identified by their phone of symmetry

41
Q

What is a Dextrorotatory

A

An Isomer that rotates plane-polarised light to the right (+)

42
Q

What is a Levorotatory?

A

An enantiomer that rotates plane-polarised light to the left (-)

43
Q

What is optically active

A

Chiral molecules that effect plane-polarised light

44
Q

What is Enantiomerically pure

A

Containing a single enantiromer

45
Q

What is a Racemic mixture?

A

A mixture with an equal amount of both enantiomers

46
Q

What is a absolute configuration

A

The exact three-dimensional structure

47
Q

What is a Pi bond?

A

A covalent bond in which the overlap regions lie above and below the internucler axis

48
Q

What is Beer-lambert’s law

A

Relates to the amount of light being absorbed to the concentration of the substance absorbing the light.

49
Q

What is dispersion force

A

Instantaneous dipole attractive force on the adjacent atom

50
Q

What is dipole-dipole force

A

A permanent dipole moment in polar molecules

51
Q

What is ion-dipole force

A

Forces between an ion and a polar molecule

52
Q

What is a solution

A

When one substance disperses uniformly throughout another.

53
Q

What is a saturated solution

A

A solution that is in equilibrium with undissolved solute

54
Q

What is a unsaturated solution?

A

Less solute that is needed to form a saturated solution.

55
Q

How do you identify a Geometric isomers?

A

They have double bond between carbon

56
Q

How do you identify optical isomers?

A

Caron surrounded by 4 different chains (Chiral)

Che144 (2 decks)

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