Midyear Flashcards

1
Q

Rutherford B. Hayes

A

Rutherford gold foil experiment. Didn’t get expected results but discovered nucleus. He predicted that the atoms would have their matter spread out like a piece of paper.

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2
Q

Atoms tend to acquire the electron configuration of….

A

A Nobel Gas

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3
Q

2 non metals

A

Both want more electrons and share with each other. This means they are molecular compounds

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4
Q

2 metals

A

No compounds

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5
Q

Metal + non metal

A

Ionic compound

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6
Q

Niels Bohr

A

Discovered only certain energies and wavelengths are allowed. INCORRECTLY thought electrons orbited nucleus

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7
Q

Quantum

A

Can be counted, NOT continuous.

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8
Q

Is light a wave or a particle?

A

Both!

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9
Q

Heisenberg uncertainty principle

A

The better you know the position, the worse you know the momentum(where it is going). NOTE this principle applies best to small (and i mean realllllly small things)

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10
Q

De Broglie wavelength

A

H/MV

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11
Q

What is an orbital?

A

A region where you are likely to find an electron (of a certain energy)

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12
Q

Sub level S

A

1 orbital, 2 electrons

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13
Q

Sub level P

A

3 orbitals, 6 electrons

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14
Q

Sub level D

A

5 orbitals, 10 electrons

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15
Q

Sub level F

A

7 orbitals, 14 electrons

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16
Q

Out of Li, Na, and K, which is most reactive and why?

A

K, it is the easiest to remove an electron so it has the lowest ionization energy

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17
Q

Ionization energy

A

The energy to move an electron

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18
Q

What is an acid?

A

Any anion with charge balanced by H+

19
Q

Anion with -ide becomes what when turned into an acid?

A

Hyrdo___ic acid

20
Q

Anion with -ate becomes what when turned into an acid?

A

__ic acid

21
Q

Anion with -ite becomes what when turned into an acid?

A

____ous acid

22
Q

Lewis dot structures

A
  • dots represent valence e- in the outermost principle energy level
  • used for non metals primarily
23
Q

Octet rule

A

All elements want 8 valence electrons (hydrogen follows the duet rule, making it the only exception)

24
Q

Covalent bonds

A

Pair of shared electrons

25
Q

VSEPR

A

Valence shell electron pair repulsion, means that outermost electron pairs repel eachother

26
Q

Difference between ammonia and ammonium

A

Ammonia: NH3. Ammonium NH4(+)

27
Q

What generally has a higher melting point, ionic or molecular compounds? Why?

A

Ionic, because the ionic bonds are much harder to break. DONT BE CONFUSED, melting point isn’t a direct comparison to the strength of the bonds

28
Q

Are acids molecular or ionic?

A

Molecular

29
Q

Redox reactions

A

The transfer of electrons:

1) synthesis
2) single displacement
3) decompositions
4) combustion (fancy word for burning)

30
Q

What makes a reaction an acid base?

A

The products are always the same, water + any salt

31
Q

Material made up of one kind of atom

A

Element

32
Q

What are the diatomic elements?

A

H, O, N, Br, I, Cl, F

33
Q

Materials made up of two or more kinds of atoms

A

Compound

34
Q

Homogenous mixture

A

A solution, same from place to place. (Ex: steel)

35
Q

Heterogenous mixture

A

Composition varies (ex:sand, salt, peanut butter)

36
Q

Physical change

A

No new substances (boiling water)

37
Q

Chemical change

A

New substances created (electrolysis) (ex:baking a cake, helps to ask if you can undo it?)

38
Q

Ion

A

A charged particle, gains and looses electrons

39
Q

What happens during alpha decay?

A

A particle joins with a Helium2 particle to form a new particle

40
Q

What happens during beta decay?

A

A particle turns one of its neutrons into a proton

41
Q

What happens during gamma decay?

A

When a particle turns one of its protons into a neutron

42
Q

J. J. Thomson

A

Discovered electrons and that all matter can emit electrons. Plum pudding model

43
Q

Cations

A

Metals that loose electrons (+)

44
Q

Anions

A

Metals that gain electrons (-)