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Gen Chem 1 > 1.1 > Flashcards

1.1 Flashcards

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1
Q

Accuracy

A

Now closely a measurement aligns with correct value

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2
Q

Properties of matter: solid

A

Has fixed shape and volume

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3
Q

Properties of matter: liquid

A

Takes shape of container

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4
Q

Properties of matter: gas

A

Expands to fill container

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5
Q

Mass vs. Weight

A

Mass: measure of the amount of matter in it

Weight: Force that gravity exerts on an object

-The weight of an object changes as the force of gravity changes, but its mass does not

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6
Q

Law of conservation of matter

A

Summarizes many scientific observations about matter

It states that there is no detectable change in the total quantity of matter present when matter converts from one type to another or changes among solid liquid or gaseous state

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7
Q

Element * physical state and composition

A

Pure substance that cannot be Brocken down into simpler substances by chemical changes

Gold, sulfur, oxygen ,copper

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8
Q

Compound * physical state and composition

A

Pure substances that are comprised of two or more elements

Orange, mercury (II) oxide, water

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9
Q

Homogenous mixture * physical state and composition

A

A mixture with a composition that varies from point to point

Italian dressing , clnoctate chip cookies, granite

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10
Q

Heterogeneous mixture * physical state and composition

A

Aka solutions exhibit uniform composition and appears visually same throughout

Air, maple syrup, gasoline, salt in water

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11
Q

Define atom

A

The smallest particle of an element that has the properties of that element and can enter into a chemical combination

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12
Q

Examples of atoms

A
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13
Q

Examples of molecules

A

molecule consists of two or more atoms joined by strong forces called chemical bonds

Water, carbon dioxide and glucose

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14
Q

Matter: does it have constant properties and composition?

A

If no, then it is a mixture

If yes, then it s a pure substance

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15
Q

Is the mixture uniform throughout?

A

Yes: homogeneous
No; heterogeneous

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16
Q

Can the pure substance be simplified?

A

No: then it is an element
Yes: then its a compound

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17
Q

Base units of the SI system:length

A

Meter (m)

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18
Q

Base unit of the si system: mass

A

Kilogram (kg)

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19
Q

Base units of the si system: time

A

Second (s)

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20
Q

Base units of the si system: temp

A

Kelvin (K)

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21
Q

base unit of the si :Electric current

A

Ampere (A )

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22
Q

Base units of the si system: amount of substance

A

Mole (mol)

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23
Q

Femto

A

f

1 f= 10^-15

1 *10^-15= 0.000000000000001

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24
Q

Pico

A

p

10^-12

1 picometer =1*10^-12 m

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25
Nano
n 10^-9 4 nanograms= 4*10^-9 grams= 0.000000004 grams
26
Nano
n 10^-9 4 nanograms= 4*10^-9 grams= 0.000000004 grams
27
Micro
10^-6 1 microliter = 1*10^-6= 0.000001 L
28
Matter
Anything that takes up space and has mass
29
Physical property
Is a characteristic of matter that is not associated with a change in its chemical composition Examples are density color hardness melting and boiling points And electrical conductivity
30
A physical change is
Change in the state of properties of matter without any accompanying change in the chemical identity of the substance is contained in the matter Example is when you observe wax melting or when steam condenses into liquid water
31
Chemical property
The ability to change from one type of matter into another or the inability to change Examples are flammability Texas City acidity and any other types of reactivity
32
Examples of chemical changes
When iron combines with oxygen in the presence of water forms to rust
33
Chemical change is
When one or more types of matter that differs from the matter present before the change
34
Extensive property vs intensive property
A drop of hot cooking oil spattered on your arm cousins brief minor discomfort we’re at a pot of hot oil fields severe burns both the drop in the part of oil are the same temperature which is an intensive property but the pot clearly contains much more heat which is extensive property
35
36
37
Using displacement of water to determine density
38
Using displacement of water to determine density
39
Precision
How closely a measurement matches the same measurement when repeated
40
Significant figures
All of the digits in a measurement, including the uncertain last digit
41
Non-zero digits are always
Significant
42
Zeros in between non-zero digits are
Significant
43
After the decimal zeros to the right of a non zero digit are
Significant
44
zeros to the left of a nonzero digit are
Not significant
45
zeros to the right of a non- zero number are always
Significant
46
Whole number ending in zero and have no decimal point are
Ambiguous
47
Sigfigs of: 26.38
4
48
Sig figs of 30006
5
49
Sig figs of 6002.1
5
50
Sig ass of 0.05070
4
51
Sigfigs of 50.000
5
52
Sigfigs of 50
1 or 2
53
Sigfigs of 50.
2
54
Sig figs of 5.0* 10^1
2
55
Sigfigs of 5 *10^1
1
56
Addition and subtraction sig fig rules
57
Multiplication and division sig figs rule
58
Multiplication and division sig figs rule
59
Add 2.334 ml and 0.31 ml
2.64 ml
60
Subtract 55.8752m from 56.533m
0.658m
61
Multiply 2.334 cm and 0.320cm
0.747 cm2
62
Mixed operation rules
63
Mixed operation rules
64
(14.115+5421.15) /14.1
65
Equation for speed
Speed = distance/ time
66
Equation for time
Time = distance/ speed
67
1 m =
1.0936 yards
68
1in=
2.54 cm
69
1 km =
0.62137 mi
70
1 mi=
1609.3m
71
1L=
1.0567 qt
72
Diatomics
Have- H2 No- N2 Fear- F2 Of- O2 Ice- I2 Cold- Cl2 BRew- Br2
73
Tetra
T 1x1012
74
Giga (G)
1 x 10^9
75
Mega (M)
1x10^6
76
Kilo (k)
1x103
77
Deci
1x10^-1
78
Centi (c)
1x10 -2
79
Milli (m)
1x10 -3
80
Micro
1x10 -6
81
Nano (n)
1x10 -9
82
Pico (p)
1x10 -12

Gen Chem 1 (1 decks)

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