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English Final > Chemistry FINAL!!!!! > Flashcards

Chemistry FINAL!!!!! Flashcards

1
Q

Mulipying and dividing Sigfigs

A

Do not round until the end
Count number of sigfigs in each number
Find the number with the lowest amount of sigfigs.

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2
Q

Sigfig rules

A

All non zero digits are significant.
Zeros between sigfigs are significant. EX (0.504)
Leading zeros are not significant
Trailing zeros after a decimal place are significant EX.(4.0)
97(2) and 97.00(4) are different
Trailing zeros can be significant, if a deciaml is shown.
Exact numbers have an infinite amount of sigfigs.
All digits that compromis “n” are significant Ex. (10^x is not significant).

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3
Q

Adding and subtracting sigfigs

A

Do not round until the end
Find number with least amount of decimal places.

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4
Q

Density equation

A

Density = Mass divided by volume

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5
Q

Physical property

A

Characteristic of a substance that can be observed without changing it to something else.

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6
Q

Chemical property

A

Characteristic of a substance that can only be observed if it is changing

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7
Q

Extensive property

A

Change based on how much matter we have
Ex. Volume, shape, mass

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8
Q

Intensive property

A

Stays the same no matter how much matter we have
Ex. Color,texture, boiling/freezing point, density

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9
Q

Mixture

A

Made of two or more pure substances

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10
Q

Element

A

Substances that cannot be seperated into simpler substances by chemical means

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11
Q

Compound

A

A pure substance composed of two or more elements whose composition is constant

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12
Q

Law of definite proportions

A

A pure substance will contain same elements in same proportions by mass

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13
Q

Alloy

A
  • Made of two or more metals, or a metal and a nonmetal (must be solid at room temp)
  • Melt solid components and allow to mix/dissolve
  • To identify must know types of metal/solid used.
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14
Q

Subscript

A

Say how many atoms of a certain element are present
If there are no subscripts then there is only 1 atom of that element.

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15
Q

Coefficient

A

Determines how many is needed
_ c2h4 + 3 o2 –> 2co2 + 2h20

c = 2
h = 4
0 = 6

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16
Q

Law of conservation of matter/mass

A

Matter cannot be created or destroyed
During chemical reactions, no matter is lost/gained
Elements you start with, you end with

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17
Q

Physical changes

A

Type of matter that has not changed
* mas, shape, volume, state of matter
Change is often reversible
*phase change, shape

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18
Q

Chemical changes

A

Type of matter that has changed into another matter
Change is often not reversible
* combustion
Generally, if the observalbe intensive properties have changed, then a chemical change has occured.

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19
Q

Reactants

A

Chemicals you start with
* CH4 + 02 —->
[________]
Reactants

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20
Q

Synthesis equation

A

A+B ——> AB

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21
Q

Decomposition equation

A

AB —–> A + B

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22
Q

Single replacement equation

A

AB + C ——> BC + A

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23
Q

Double replacement equation

A

AB + CD —–> AD + CB

24
Q

Combustion equation

A

C x Hy + o2 —-> CO2 + H2O

25
Q

Synthesis identification

A

Count reactants and products, start with 2, end with 1

26
Q

Decomposition identification

A

Count reactants and products, start with 1, end with 2

27
Q

Single replacement identification

A

You will have a pure element on BOTH sides of the equation

28
Q

Double replacement identification

A

Second element of each compound swap

29
Q

Combustion identification

A

A hydrocarbon oxygen gas are always the reactants because h2O is always a product

30
Q

Know how they drew the atom Jj thompson

A

insert picture here

31
Q

Know how they drew the atom Erwin shrodinger

A

insert picture here

32
Q

Know how they drew the atomLouis Debrogile

A

insert picture here

33
Q

Know how they drew the atom Bohr

A

insert picture here

34
Q

Know how they drew the atom John Dalton

A

insert picture here

35
Q

know how the drew the atom Democritus

A

insert picture here

36
Q

Robert milikan

A

Oil drop
* discovered mass/ change of electron
*change: 159 ^ 10-19
*Mass: 9.13 ^10-31 kg

37
Q

Cathode tube ray experiment discovery

A

An electron is a subatomic particle that is found in all atoms, is negatively charged, and has extremely small mass (200 * lighter than a hydrogen atom).

38
Q

Alpha particles

A

2 protons, 2 nuetrons
Mass number: 4 amu
Charge: +2

39
Q

Beta particles

A

Electrons
Mass number: 0
Charge: -1

40
Q

Gamma radiation

A

High energy proton with short wavelengths
Mass number: 0
Charge: 0

41
Q

Alpha decay

A

233 -4 229 4
NP ———> PA + He
93 -2 91 2

42
Q

Beta decay

A

40 0 40 0
K —–> Ca e-
19 +1 20 -1

43
Q

Valence electrons

A

-Found in the highest energy level of an atom
- Responsible for bonding properties of an atom

44
Q

Rule 1 for lewis dot structure

A

Write element symbol

45
Q

Rule 2 for lewis dot structure

A

Figure out how many valence electrons you need

46
Q

Rule 3 for lewis dot structure

A

Draw dots to represent electrons along the symbol
Draw on “4 sides”, order does not matter
Every side needs 1 electron before pairs

47
Q

Wavelength

A

Distance between 2 adjacent crests or troughs

48
Q

Frequency

A

Number of waves that pass through a given point per second

49
Q

Photoelcetric effect

A

WHen a metallic surface is exposed to radiation of a certain frequency, electrons can be emitted

50
Q

Electron configuration

A

Shows an arrangement of electrons in an atoms and shows how electrons are distributed in orbital

51
Q

Lavoisier

A

Made first list of 33 elements

52
Q

J.W. Dobereiner

A

Arranged known elements into triads

53
Q

John newlands

A

Arranged by increasing atomic mass

54
Q

Mendeleev and Lothar meyer

A
  • Ordered 63 elements by increasing atomic mass
  • Left space for unknown elements
55
Q

Moseley

A

Organized by atomic number instead of mass

English Final (20 decks)

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