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sch 4u > Atomic Structures and Properties > Flashcards

Atomic Structures and Properties Flashcards

1
Q

Democritus’ theory

A

All matter is made up of indivisible particles called “atoms” and void, which is the empty spaces between atoms

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2
Q

John Dalton’s Theory

A
  • Atoms are indivisible and can’t be broken down
  • all matter is made up of tiny particles
  • all atoms of one element are are identical
  • atoms create compounds by combining atoms of different elements
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3
Q

JJ Thomson’s Theory

A
  • Cathode rays of negative charge, that were deflected by a magnetic field & how much energy they carry
  • atom is really a positive field with negative charges embedded within it’s matrix (raisin bun)
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4
Q

The Rutherford model

A

conducted the alpha particle experiment (gold foil)

  • most particles went through
  • a small fraction had a large deflection
  • a minute fraction rebounded
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5
Q

Rutherford’s nuclear atom model

A
  • atom is mostly empty space
  • All positive charge is concentrated in a small volume called the nucleus
  • electrons revolve around the nucleus like planets in the solar system
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6
Q

Plank / Einstein - Quantum

A
  • plank determined that energy is absorbed by atoms in certain fixed amounts known as quanta
  • Einstein extended the theory by determining that radiant energy is also quantized
  • discrete energy packets = photons
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7
Q

Einsteins theory

A

electromagnetic radiation has characteristics of both a wave and a stream of particles

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8
Q

The Bohr model

A
  • Electrons revolve around the nucleus in certain allowed orbits; each orbit corresponds to a specific amt of EN
  • As long as the electron remains in the same orbit, it neither emits nor absorbs EN
  • As the electron jumps from one orbit to another, EN is absorbed or emitted
  • EN difference between orbits corresponds to specific wavelengths
  • Bohr’s calculations only worked for hydrogen
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9
Q

DeBroglie (wave mechanical model)

A

-understanding that any small particle, such as an electron in motion, has associated wave behaviour

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10
Q

Schrodinger (wave mechanical model)

A
  • considered the behaviour of the inside of an atom
  • The positive nucleus is surrounded by a cloud of electrons waves, electrons can only have quantized energy levels because the requirement for whole # of wavelengths for electron waves
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11
Q

Heisenberg uncertainty principle (wave mechanical model)

A

-impossible to know both the velocity and location of an electron at the same time

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12
Q

S orbital

A
  • Spherical in shape
  • size increases as “n” increases
  • There is only 1 S orbital in a sublevel
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13
Q

P orbital

A
  • Dumb-bell shaped
  • Aligned along x, y, z axis
  • only 3 p orbitals in a sublevel
  • size increases as “n” increases
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14
Q

D orbital

A
  • has 4 lobes per orbital
  • aligned according to x, y, z axis
  • only 5 d orbitals in a sublevel
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15
Q

F orbital

A
  • don’t need to know the shape

- only 7 f orbitals in a sublevel

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16
Q

Principal quantum number (n)

A

-ENERGY LEVEL
refers to the major (or principal) energy levels in an atom
-the higher n is the farther away the electrons are from the nucleus

17
Q

Angular momentum number (l)

A 
-SUBLEVEL (S, P, D, F)
energy sublevel
-shape of orbital 
-l = n - 1 
0 = s 
1 = p
2 = d 
3 = f
18
Q

Magnetic quantum number (ml)

A

-ORBITAL ORIENTATION
Orientation of the orbital
-specifies the exact orbital within each sublevel
-l to +l example: l = 2 ml = -2, -1, 0, 1, 2

19
Q

Spin quantum number (ms)

A

-SPIN OF ELECTRON
Electron spin +1/2 -1/2
an orbital can hold 2 electrons that spin in opposite directions

20
Q

Pauli exclusion principal

A
  • no two electrons in an atom can have the same 4 quantum numbers
  • each electron has a unique address
  • Change of spin on electron
21
Q

Aufbau principal

A

each electron goes into the lowest available energy state, once that is full the next lowest starts filling

22
Q

Hund rule

A

bus seat principal
-orbitals with the same energy levels (three 2p) electrons will occupy all empty orbitals first before a second electron goes into the orbitals

23
Q

Atomic size

A
  • down the periodic table the size increases (more energy levels, and inner electrons shielding the nucleus)
  • across the periodic table the size decreases (more protons inside the nucleus, electrons pulled inwards)
24
Q

Ionization energy

A
  • The amount of energy required to pull off an electron
  • decrease as you go down (easier to pull an electron off a bigger atom)
  • increase as you go across (more difficult to remove an electron off of a smaller atom)
25
Q

Electron Affinity

A

the measure of change in energy that occurs when an electron is added to the outer energy level to form an anion

  • decreases down (the effect of the nuclear charge will not have as great of an effect on a large atom)
  • increases across (effect will be greater on smaller atoms)
26
Q

What elements can have less than 8 electrons for a stable octet?

A

Hydrogen
Boron
Beryllium

27
Q

What elements can have more than 8 electrons for a stable octet?

A

Sulfer
Phosphorus
Xenon

28
Q

What does VSEPR stand for?

A

Valence Shell Electron Pair repulsion theory

29
Q

Linear

A

2 total bonds
2 bonds = linear (180)
2 lone pairs = linear (180)

30
Q

Trigonal Planar

A

3 total bonds
3 bonds, 0 lone = trigonal planar (120)
2 bonds, 1 lone = bent (<120)
1 bond, 2 lone = 120

31
Q

Tetrahedral

A 
4 total bonds 
4 bonds, 0 lone = Tetrahedral (109.5)
3 bonds, 1 lone = Trigonal pyramidal (107)
2 bonds, 2 lone = bent (104.5) 
3 bone, 1 lone = linear (180)
32
Q

Trigonal Bipyramidal

A 
5 total bonds 
5 bonds, 0 lone = trigonal bipyramidal (120/90)
4 bonds, 1 lone = See-saw 
3 bonds, 2 lone = T shaped 
2 bonds, 3 lone = Linear 
1 bond, 4 lone = Linear
33
Q

Octahedral

A 
6 total bonds (90)
6 bonds, 0 lone = octahedral 
5 bonds, 1 lone = square based pyramidal 
4 bonds, 2 lone = square planar 
3 bonds, 3 lone = t shaped 
2 bonds, 4 lone = linear 
1 bond, 5 lone = linear
34
Q

Intramolecular

A

forced within the molecule, much stronger than inter molecular

35
Q

Intermolecular

A

forces between molecules

36
Q

Properties of Ionic solids

A
  • Brittle
  • conduct electricity in liquid form or solution (not solid)
  • high melting point
37
Q

Properties of metallic solids

A
  • electrical conductors
  • malleable / ductile
  • high melting point
38
Q

properties of small molecular solids

A
  • low melting point
  • not very hard
  • non conductors
39
Q

Properties of covalent network crystals

A
  • extremely hard
  • brittle
  • very high melting point
  • non conductors (except graphite)
  • insoluble

sch 4u (1 decks)

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