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Chemistry 121 A > Chapter 1: matter and measurement > Flashcards

Chapter 1: matter and measurement Flashcards

0
Q

What is matter

A

Matter is anything that has mass and takes up space

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1
Q

What is chemistry

A

We study matter, it’s properties, and it’s behavior

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2
Q

What is an atom

A

Building blocks of matter

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3
Q

What is an element

A

Made up of the same kind of atom that cannot be decomposed into smaller substances

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4
Q

What is a compound

A

Two or more different kinds of elements

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5
Q

Why do we study chemistry

A

Chemistry is a central science, central to the fundamental understanding of other sciences and technologies involved in everything we do

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6
Q

What is the conversion factor for 1in to mm then to cm

A

1in=25.40mm=2.540cm

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7
Q

What is 1yd to cm then to m

A

1yd=91.44cm=0.9144m

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8
Q

What is 1ft to in to cm to m

A

1 ft=12in=30.48cm=0.3048m

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9
Q

What is 1mi to km to m

A

1mi=1.609km=1609m

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10
Q

What is 1lb to g to kg

A

1lb=453.6g=0.4536kg

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11
Q

What is 1oz to g to mg

A

1oz=28.35g=2835mg

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12
Q

What is 1gal to L to ml to cm3

A

1gal=3.785L=3785ml=3785cm3

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13
Q

What is a pure substance

A

It is a matter that has distinct properties and composition does not vary from sample to sample

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14
Q

What is a mixture

A

The composition of two or more substances that retain their identity. A physical blend of two or more substances

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15
Q

What is a homogenous mixture

A

It is a mixture that is uniform throughout

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16
Q

What is a heterogeneous mixture

A

A mixture that is not uniform throughout

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17
Q

What is the physical property of matter

A

It can be observed without changing a substance into another substance

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18
Q

What are some examples of physical properties

A

Boiling point, density, volume, and changes of state

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19
Q

What is a chemical property

A

It can only be observed when a substance is changed into another substance

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20
Q

What are some examples of chemical properties

A

Flammability, corrosiveness, and reactivity

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21
Q

What is an intensive physical property

A

They are independent of the amount of the substance that is present

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22
Q

What are some examples of intensive properties

A

Density, boiling point, and color

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23
Q

What is an extensive property

A

It depends on the amount of the substance present

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24
What are some examples of extensive properties
Mass, volume, and energy
25
What is a chemical reaction
In the case of a chemical reaction, the reacting substances are converted to new substances
26
What is filtration.
Solid substances are separated from liquids and other substances
27
What is distillation.
Uses differences in boiling points of substances to separate a homogeneous mixture into its components
28
What is chromatography.
It separates substances on the basis of differences in solubility in a solvent
29
What is the SI unit for mass, length, temperature, amount of substance, and time
``` Kilogram-kg Meter-m Kelvin-k Mole-mol Second-sec ```
30
What is mass.
The measure of the amount of matter in an object
31
What is weight.
The measure of the gravitational force on the matter in an object
32
What is temperature.
A measure of the hotness or coldness of an object. It is a physical property that determines he direction of heat flow. Flows from high to low temperature. Temperature is the measure of the average kinetic energy of the particles in a sample.
33
What is the equation for the kelvin
K= C+273.15
34
What is the equation for Fahrenheit
F=9/5(C) +32
35
What is the equation for Celsius
C=5/9(F-32)
36
What is the freezing point of each temperature unit
32F=0C=273K
37
What are the boiling points of each of the temperature units
212F=100C=373K
38
What is a derived unit
A unit of measurement that is determined by combining one or more measurements
39
What are the most commonly used units in volume
L and mL
40
What is density.
A physical property of a substance that has units (g/mL) that are derived from the units of mass and volume
41
What is an exact number
Known as counting or defined
42
What is an in exact number
Derived from measurements.
43
What is accuracy.
Refers to the proximity of a measurement to the true value of a quantity
44
What is precision.
Refers to the proximity of several measurements to each other
45
What is the Atomic theory of matter
1. Each element is composed of extremely small particles called atoms 2. All atoms of a given element are identical to one another in mass and other properties, however the atoms of one element are different from atoms of all other elements 3. Atoms of an element can't be changed into atoms of another element by chemical reactions, atoms are neither created nor destroyed in chemical reactions 4. Compounds are formed when atoms of more than one element combine, a given compound always has the same relative number and kind of atoms
46
What is the law of conservation of mass
The total mass of substance present at the end of a chemical process is the same ad the mass of substance present before the process took place
47
What is the atomic number
The number of protons or electrons. It is the same for each element
48
What is the mass number
The total number of protons and neutrons in the atom
49
What are isotopes.
Atoms of the same element with different masses. They have different number of neutrons
50
What is the average atomic mass
Calculated from the isotopes of an element weighted by their relative abundance a (Isotope mass) times (fractional isotope abundance)
51
What are the horizontal lines in a periodic table and how many are there
They are periods and there are 7
52
What are the vertical columns on the periodic table and how many are there
They are groups containing the same properties and there are 18
53
What are the five groups
1. Alkali metal 2. Alkaline Earth Metal 3. Chalcogens 4. Halogens 5. Noble gases
54
What are the Alkali metals
Li, Na, K, Rb, Ca, and Fr
55
What do the subscript to the right if the symbol mean
Tells the number of atoms of that element in one molecule of the compound
56
What are molecular formula
Gives the exact number of atoms of each element in a compound
57
What is empirical formula
Gives the lowest whole-number ratio of atoms of each element in a compound
58
What are structural formulas
Shows the order in which atoms are bonded.
59
What are molecular compounds
Composed of molecules and almost always contain no metals
60
What are diatomic molecules
These are seven elements that occur naturally as molecules containing two elements 1. Hydrogen 2. Oxygen 3. Nitrogen 4. Fluorine 5. Chlorine 6. Bromine 7. Iodine
61
What are ions.
When atoms gain or lose electrons, the become ions
62
What are cations.
Positive and formed by elements on the left side of the periodic chart
63
What are anions.
Negative and are formed by elements on the right side o the periodic chart
64
What are ionic compounds
Generally a combination of metals and no metals
65
Rules for inorganic nomenclature
- Write the name of the cation - if the anion is an element, change it's ending to -ide, if the anion is a polyatomic ion, write its name. - if the cation has more than one possible charge, write he charge as a Roman numeral
66
Patterns in oxyanion nomenclature
When there are two oxyanions involving the same element - the one with fewer oxygens ends it -ite - the one with more oxygens ends in -ate

Chemistry 121 A (1 decks)

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