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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

A

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

24
Q

certain digits

A

given by the smallest grid

25
Q

uncertain digit

A

by estimate

26
Q

precision of a measurement depends on the?

A

instruments

27
Q

the uncertain digits is always the?

A

right most digit

28
Q

significant figures

A

the digits in any measurement that are known with certainty plus 1 digit that is uncertain (estimate digit)

29
Q

sig fig - multiplication and division

A

answer should contain the same number of sig fig as the measurement with the least number of significant digits

30
Q

sig fig - +/-

A

answer many not have any more decimal places than the least accurate number

31
Q

exact numbers

A

counting
definition
unit conversion

32
Q

measure number

A

obtained by using instruments

33
Q

Density

A
  • the ratio between mass and volume

D = M/V

34
Q

periodic table

A
  • graphical display of elements
  • elements are arranged by increasing atomic number
  • elements with similar properties are placed in same column of the display
35
Q

periodic table: rows and column

A
  • 7 rows: 7 periods

- 18 columns: 18 groups (8 group a and 10 group B)

36
Q

major groups in the period table

A
  • 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
Q

alkali metals

A
  • 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
Q

Alkali Earth Metals

A
  • 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
Q

Group 7A: Halogens

A
  • 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
Q

Group 8A Noble gas

A
  • chemically very stable
  • rarely react with other elements
  • exist in nature as odorless, colorless monoatomic gases
40
Q

different parts of periodic table which are located at different parts

A
  • metals
  • non metals
  • metalloids
41
Q

metals

A
  • left side of zigzag
  • except Helium (non metal)
  • shiny, ductile, malleable
  • good conductor
  • high melting points
  • high density
42
Q

metalloids

A
  • zigzag border separating metals and non metals
  • blue-gray, shiny
  • brittle, easily shattered
  • poor conductor
  • medium melting points
  • medium density
43
Q

nonmetals

A
  • right of zigzag point
  • dull
  • brittle, easily shattered
  • poor conductor
  • lower melting points
  • lower density
44
Q

physical state of elements

liquid

A

Mercury and Bromine

45
Q

proton

A

charge of +1
mass of 1 amu
in nucleus

46
Q

neutron

A

charge of 0 or neutral
mass of 1 amu
located in nucleus

47
Q

electron

A

electrical charge of -1
mass of .0005 amu
located in: dispersed through out electron cloud; not in nucleus

48
Q

amu

A

atomic mass unit

49
Q

atomic number of an element

A

Z

  • ID # of the element
  • number of the proton
50
Q

what is an element

A

pure substance in which all atoms present have the same atomic number

51
Q

Z

A

of both p+ and e-

52
Q

isotopes

A

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
Q

mass number

A

symbol A

A = p+ + nº

54
Q

isotope symbol

A 
A
  E
Z
A= mass
E = atomic symbol
Z = electron
55
Q

weighted average mass

A
  • 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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