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Chemistry > Powerpoint Exam 1 > Flashcards

Powerpoint Exam 1 Flashcards

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1
Q

chemistry

A

study of the composition properties and interactions of matters

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2
Q

elements

A 
building blocks (alphabets) of matters
- pure substances that cannot be separated into simpler substances by ordinary laboratory process
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3
Q

example of elements

A

oxygen, hydrogen, carbon, gold

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4
Q

building blocks of matter

A

1 oxygen + 2 hydrogen –> water

1 carbon + 2 oxygen –> carbon dioxide

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5
Q

as of 2007 how many known elements are there and how many can be found in nature?

A

117 known elements

- 94 can be found in nature

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6
Q

the elemental substance

A
  • each element has it sown unique physical and chemical properties
  • each has its own name
  • some are named for their appearance, others for planets, mythological figures, scientists, or places
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7
Q

symbols of elements

A

consists of 1 or 2 leters

- Capital and lower case

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8
Q

particular nature of matters

A
  • macroscopic
  • submicroscopic
  • macroscopic
  • properties and interactions of submicroscopic particles of atoms and molecules determines the properties and behaviors of matter we experience and observe macrocopicly
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9
Q

three terms for the submicroscopic particles

A

atoms
molecules
ions

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10
Q

atom

A

smallest particle of an element that can exist and still have chemical properties of the element

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11
Q

molecules

A

2 or more atoms joined together in a specific arrangement

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12
Q

ions

A

atoms or a group of bonded atoms with an electrical charge

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13
Q

all atoms of a given elements are?

A

identical

- the atoms of a given element are different from those of any other element

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14
Q

what is the basic unit for chemical changes/chemical reactions?

A

atom

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15
Q

molecular view of an element

A

one type of atoms in each elements

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16
Q

molecules

A
  • group of two or more atoms joined in a specific geometrical arrangement and behave like a single unit
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17
Q

classify molecules by the number of atoms

A
  • Diatomic molecule
  • triatmic
  • tetratomic
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18
Q

classify molecule by the type of attoms

A

homoatomic molecules

heteroatomic molecules

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19
Q

homoatomic

A
  • molecules in which all atoms present are of the same kind

- pure substance containing homoatomic molecules must be an element

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20
Q

heteroatomic molecules

A
  • molecules in which two or more kinds of atoms are present

- a pure substance containing heteroatomic molecules must be compounds

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21
Q

what is matter? and example

A

matter is anything which has mass and takes up space (volume)

ex: sand (solid)
- water (liquid)
- air (mixture of gases)
- human body (solid, liquid, gas)

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22
Q

what kind science is chemistry?

A

empirical science

- based on the results of experiments/observations

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23
Q

common types of measurements in chemistry

Study These Flashcards
A

Length - m
Mass - g
Volume - L
Time - duration of experiment or observation

24
Q

certain digits

Study These Flashcards
A

given by the smallest grid

25
uncertain digit
by estimate
26
precision of a measurement depends on the?
instruments
27
the uncertain digits is always the?
right most digit
28
significant figures
the digits in any measurement that are known with certainty plus 1 digit that is uncertain (estimate digit)
29
sig fig - multiplication and division
answer should contain the same number of sig fig as the measurement with the least number of significant digits
30
sig fig - +/-
answer many not have any more decimal places than the least accurate number
31
exact numbers
counting definition unit conversion
32
measure number
obtained by using instruments
33
Density
- the ratio between mass and volume | D = M/V
34
periodic table
- graphical display of elements - elements are arranged by increasing atomic number - elements with similar properties are placed in same column of the display
35
periodic table: rows and column
- 7 rows: 7 periods | - 18 columns: 18 groups (8 group a and 10 group B)
36
major groups in the period table
- alkali metals (1st column - except for helium) - alkali earth metals (2nd column) - transition metals (3-12th column) - halogens (2nd to last column or 17th) - noble gases ( last column) - inner transition metals (the ones separated)
37
alkali metals
- group 1A - silver colored, soft, low density metals - chemically highly reactive, rarely found in elemental form in nature - reacts strongly with water to form base-alkali metal
38
Alkali Earth Metals
- Group 2A - harder, higher melting, and denser than alkali metals - reactive, but less than corresponding alkali metal - form stable, insoluble oxides from which they are normally extracted - oxides are basic - alkaline earth
38
Group 7A: Halogens
- chemically highly reactive - found in nature only in compounds or as ions - the elemental forms are made in laboratory - each element exist as diatomic molecules - only group exhibiting all 3 states at room temperature: - - F2, Cl2 = gas - - Br2 = liquid - - I2 = Solids
39
Group 8A Noble gas
- chemically very stable - rarely react with other elements - exist in nature as odorless, colorless monoatomic gases
40
different parts of periodic table which are located at different parts
- metals - non metals - metalloids
41
metals
- left side of zigzag - except Helium (non metal) - shiny, ductile, malleable - good conductor - high melting points - high density
42
metalloids
- zigzag border separating metals and non metals - blue-gray, shiny - brittle, easily shattered - poor conductor - medium melting points - medium density
43
nonmetals
- right of zigzag point - dull - brittle, easily shattered - poor conductor - lower melting points - lower density
44
physical state of elements | liquid
Mercury and Bromine
45
proton
charge of +1 mass of 1 amu in nucleus
46
neutron
charge of 0 or neutral mass of 1 amu located in nucleus
47
electron
electrical charge of -1 mass of .0005 amu located in: dispersed through out electron cloud; not in nucleus
48
amu
atomic mass unit
49
atomic number of an element
Z - ID # of the element - number of the proton
50
what is an element
pure substance in which all atoms present have the same atomic number
51
Z
of both p+ and e-
52
isotopes
atoms of the same element with different numbers of neutrons (mass of an atom) - same element with different mass - same number of electrons - same chemical properties
53
mass number
symbol A | A = p+ + nº
54
isotope symbol
``` A E Z A= mass E = atomic symbol Z = electron ```
55
weighted average mass
- the observed atomic mass for an element is the weighted average mass, based on the weight of each individual isotope

Chemistry (17 decks)

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