Chapter 1 Flashcards by Does Not Matter

What was the Greeks view of chemistry?

Everything was made of:
-earth
-water
-air
-fire

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What is alchemy (who are alchemists)?

The process of concerting base metals (common and relatively abundant metals) into noble metals (metals of high value for their properties)

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Chemistry exists at the center of the __________ Universe?

STEM

Review slide 5 of chapter one

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3 examples of chemistry in everyday life?

-Metabolic reactions in the body

-Synthesizing polymers for producing medical devices

-Refining crude oil into petroleum products

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What are the three most common states of matter? What are the properties of each phase?

Solid: rigid and possesses a definite shape

Liquid: flows and takes the shape of its container

Gas: takes both the shape and volume of its container

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What is matter?

Matter is anything that occupies space and has mass

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What is an additional phase of matter?
Describe this phase?
Give examples?

Plasma: a gaseous state of matter that contains an appreciable amount of electrically charged particles

Has distinct properties c.f. (compare), ordinary gases

Plasma found in certain high temperature environments:

Naturally: stars, lightning
Man-made: television screens

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Describe mass verses weight?

Mass is a measure of the amount of matter in an object

Weight refers to the force that gravity exerts on an object

(same mass on the moon but different weight)

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What is The Law of Conservation of Matter?

There is no detectable change in the total quantity of matter present when matter converts from one type to another
(True for both physical and chemical changes)

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What is an element?

How many known?
How many occur naturally?
How many created in labs?

An element is a type of pure substance that cannot be broken down into simpler substances by chemical changes

The known elements are displayed in the periodic table:
-More than 100 known elements
-90 occur naturally
-two dozen have been created in labs

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What is a pure substance?
What two categories can pure substances be broken down into?
Describe these categories?

Substances that have a constant composition.

Elements: pure substance that cannot be further broken down into simpler substances through chemical change
Consists of just a single type of element
Egs., Au (gold), P (phosphorus), O (oxygen)

Compounds: pure substances that can be broken down into simpler substances through chemical change
Consists of ≥ 2 types of elements that are chemically bonded
Egs., H2O, C6H12O6, AgCl
Compounds differ in terms of chemical and physical properties compared to the elements from which they are formed

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What is a mixture?
What two categories exist for mixtures?
Describe these categories?

A mixture is composed of ≥ more types of matter that can be present in varying amounts; and, can be separated via physical changes

Homogenous mixture: the components of the mixture are not discernable (Gatorade)

Heterogenous mixture: individual components are discernable (salad dressing)

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Classification of matter tree?

See slide 16 in chapter one

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What is an atom?

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

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Who first proposed the idea of atoms?

Idea first proposed by Greek philosophers, Leucippus and Democritus, in the 5th century BCE

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Who provided support for the atom proposition?

19th century, John Dalton of England supported this hypothesis with quantitative measurements

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What is a molecule?

Molecule: Consists of two or more atoms connected by strong forces known as chemical bonds

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What are the three domains of chemistry?

Macroscopic
Microscopic
Symbolic

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Almost _________ of naturally occurring elements are used to make a cell phone.

one-third

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The characteristics that enable us to distinguish one substance from another are called ________.

What are the two types of this?

Properties

Physical and chemical properties

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What is a physical property?
Examples?

A physical property is a characteristic of matter that is not associated with a change in its chemical composition.

Examples: density, color, hardness, melting and boiling points, and electrical conductivity

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What is a physical change?

A physical change is a change in the state or properties of matter without any accompanying change in its chemical composition.

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What is a chemical property?
Examples?

The change of one type of matter into another type (or the inability to change) is a chemical property.

Examples: flammability, toxicity, acidity, reactivity, and heat of combustion.

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What are extensive properties?
Examples?

Property of a substance that
depends on the amount of the substance

Examples: mass, volume, heat

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What are intensive properties? Examples?

Property of a substance that is independent of the amount of the substance Examples: density, temperature

________ provide the information that is the basis of most of the hypotheses, theories, and laws in chemistry.

Measurements

What three kinds of information does each measurement provide?

Every measurement provides three kinds of information: 1. The size or magnitude of the measurement: a number 2. A standard of comparison for the measurement: a unit 3. An indication of the uncertainty of the measurement.

What system of units is used in chemistry?

In chemistry, we use an updated version of the metric system known as the International System of Units, or SI units. (Used since 1964)

Unit of length?

meter (m)

Unit of mass?

kilogram (kg)

Unit of time?

Second (s)

Unit of temperature?

Kelvin (K)

Unit of electrical current?

Ampere/Amp (A)

Unit of amount?

Mole (mol)

Unit of luminous intensity?

Candela (cd)

How was the meter length created?

The meter was originally intended to be 1/10,000,000 of the distance from the North Pole to the equator. A meter is now defined as the distance light travels in a vacuum in 1/299,792,458 of 1 second.

A meter is about ____ inches longer than 1 yard.

How was kilogram mass determined?

A kilogram was originally defined as the mass of a liter of water. It is now defined by a certain cylinder of platinum-iridium alloy, which is kept in France.

1 kilogram is about _____ pounds

2.2

Compare Celsius and Kelvin? Symbol needed? Allowed in SI system? Scale comparison? Freezing and boiling points of water?

No degree word nor symbol (°) is used with kelvin but one is used in Celsius. The degree Celsius (°C) is also allowed in the SI system. Celsius degrees are the same magnitude as those of kelvin, but the two scales place their zeros in different places. Water freezes at 273.15 K (0 °C) and boils at 373.15 K (100 °C).

What is volume and what are the SI units of volume?

Volume: The measure of the amount of space occupied by an object. The standard SI unit for volume is the cubic meter (m3), which is derived from the SI base unit of length. Other units for volume are the liter (L) and milliliter (mL). 1 dm3 = 1 L 1 cm3 = 1 mL

What is density? Equation? SI unit?

The density of a substance is the ratio of the mass of a sample of the substance to its volume. density = mass / volume The standard SI unit for density is the kilogram per cubic meter (kg/m3). Commonly used density units based on state of matter: g/cm3 (solids, liquids) g/L (gases)

____ is the only type of measurement that is free from uncertainty.

Counting

The result of a counting measurement is an example of an ____ ____?

Exact number

What are 3 common exact numbers?

The numbers for defined quantities are also exact. 1 ft. is exactly 12 in. 1 in. is exactly 2.54 cm 1 g is exactly 0.001 kg

Quantities derived from measurements other than counting are ___________________________________. Which means they are not _________.

Quantities derived from measurements other than counting are uncertain to varying extents Exact

There are always ____ ____ of the measurement process used. A measured number must be reported in a way to indicate its ____. In general, when recording a measurement, you are allowed to estimate ___________.

There are always practical limitations of the measurement process used. A measured number must be reported in a way to indicate its uncertainty. In general, when recording a measurement, you are allowed to estimate one uncertain digit.

All the digits in a measurement, including the uncertain last digit, are called ____ ____ or ____ ____?

Significant figures or significant digits

Frequently, we need to know the number of ____ ____ in a measurement reported by someone else.

significant figures or significant digits

Which numbers are always significant?

These numbers are always significant. Nonzero digits -Captive zeros -Trailing zeroes When they are to the right of the decimal place When in scientific notation

When are numbers not significant?

These numbers are always not significant. -Leading zeros -Trailing zeros When they are to the left of the decimal place

Rule of adding or subtracting?

When we add or subtract numbers, we should round the result to the same number of decimal places as the number with the least number of decimal places (the least precise value in terms of addition and subtraction).

Rule of multiplying or dividing?

When we multiply or divide numbers, we should round the result to the same number of digits as the number with the least number of significant figures (the least precise value in terms of multiplication and division).

Rule of rounding (for this class)?

if it is 5 round up.

Results calculated from measured numbers are at least as ____ as the measurement itself

Uncertain

A measurement is said to be ____ if it yields very similar results when repeated in the same manner.

Precise

A measurement is considered ____ if it yields a result that is very close to the true or accepted value.

Accurate

A quantity of interest may not be easy (or even possible) to measure directly but instead must be calculated from other directly measured properties and appropriate mathematical relationships. The mathematical approach we will be using is known as ____ ____?

Dimensional analysis

What is dimensional analysis based on?

Dimensional analysis is based on the premise that the units of quantities must be subjected to the same mathematical operations as their associated numbers

A ____ ____ or ____ ____ ____ is a ratio of two equivalent quantities expressed with different measurement units.

conversion factor or unit conversion factor

What does temperature refer to?

Temperature refers to the hotness or coldness of a substance.

Describe the Fahrenheit scale relative to the Celsius scale?

Celsius scale Water freezes at 0 °C. Water boils at 100 °C. Fahrenheit scale Water freezes at 32 °F. Water boils at 212 °F. 100 °C covers the same temperature interval as 180 °F.

Chapter 1 Flashcards

(62 cards)