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Chemistry 1 > Exam 1 Review > Flashcards

Exam 1 Review Flashcards

1
Q

Classify the basic forms of matter.

A

Solid, liquid, gas.

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2
Q

Identify the types of pure substances.

A

Elements and compounds.

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3
Q

Physical property.

A

Observed without changing the composition or identity of a substance.

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4
Q

Physical change.

A

Produces a recognizable difference in the appearance of a substance, without causing any change to its composition.

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5
Q

Example of physical changes (simple).

A

Phase change

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6
Q

What are examples of physical properties?

A

Conductivity, boiling point, density, temperature, volume, solubility.

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7
Q

What are examples of chemical properties?

A

Flammability, oxidation state, acidity.

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8
Q

Define intensive properties.

A

Properties of matter that are independent of quantity.

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9
Q

Examples of intensive properties.

A

Color, melting point, boiling point, don’t ask me about density.

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10
Q

Examples of extensive properties.

A

Mass, volume.

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10
Q

Define extensive properties.

A

Properties of matter that are dependent on the quantity.

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10
Q

Significant figure rules.

A

All nonzero digits are significant. Zeros located between nonzero digits are significant. Trailing zeros are significant if the number has a decimal point. Zeros to the left of the nonzero digit are insignificant.

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11
Q

Significant figure rules in addition/subtraction.

A

The result cannot have greater significance than any of the quantities that produced the result.

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11
Q

Accuracy

A

Degree of agreement between the true value and measured value.

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11
Q

When adding or subtracting in scientific notation…

A

Convert both numbers to standard form.

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11
Q

Significant figure rules in multiplication/division.

A

The result should have the same amount of significant figures as the number with the least significant figures.

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11
Q

Conversion between Celsius and Fahrenheit.

A

F = 1.8 x C + 32

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11
Q

Precision

A

Degree of agreement between all measures values.

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11
Q

Density formula.

A

d = m / v (g/ml or g/L)

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12
Q

Define specific gravity, give the formula.

A

Specific gravity is the ratio of the density of a substance to the density of water.
Specific gravity =
density of object / density of water

13
Q

What element is most present in the human body?

A

Oxygen.

14
Q

Groups vs. Periods

A

Groups are vertical! Periods are horizontal.

15
Q

A neutral atom has…

A

The same number of electrons and protons.

16
Q

Atomic number (Z).

A

The number of protons in an atom.

17
Q

Mass number (A).

A

Sum of the protons and neutrons in an atom.

18
Q

The letter for the atomic number is…

A

Z

19
Q

The letter for the mass number is…

A

A

20
Q

Define isotopes.

A

Atoms of the same element with different numbers of neutrons, therefore a different mass number.

21
Q

Do isotopes have identical chemical properties?

A

Yes.

22
Q

Atomic mass is the…

A

Weighted average of all the isotopes of a specific element.

23
Q

Steps to find atomic mass, given mass number of isotopes and percentages.

A
  1. Convert percentages to decimals (e.g. 75.77% –> 0.7577)
  2. Multiple the decimal by the mass of the associated isotope (e.g. 0.7577 x 35 = 26.5)
  3. Do this for all the given isotopes.
  4. Add them all together!
24
Q

Dalton’s Atomic Theory (postulates).

A
  1. TRUE All matter is made up of atoms.
  2. An atom cannot be created, destroyed, or converted to another kind of atom.
  3. Atoms of a particular element have identical properties.
  4. TRUE Atoms of different elements have different properties.
  5. TRUE Atoms of different elements combine in simple, whole-number ratios to form compounds.
  6. TRUE Chemical change involves joining, separating, or rearranging atoms.
25
Q

What postulates are still regarded as true?

A

1,4,5,6.

26
Q

What experiment provided proof of electrons?

A

Cathode-ray.

27
Q

What experiment provided proof of the nucleus?

A

Gold-foil.

28
Q

Law of Conservation of Mass.

A

In a chemical reaction, matter is neither created nor destroyed. The total mass of the substances involved does not change.

29
Q

Law of Definite Proportions

A

All samples of a given compound have the same proportions of their constituent elements.

30
Q

Law of Multiple Proportions

A

When two elements form two different compounds, the masses of the constituent elements can be expressed as a ratio of whole numbers.

31
Q

Elements of the same… have similar properties.

A

Group.

32
Q

Metals tend to…

A

lose electrons.

33
Q

Nonmetals tend to…

A

gain electrons.

34
Q

Metalloids have…

A

properties intermediate between metals and nonmetals.

35
Q

The properties of metals are…

A

Solid at room temperature, highly malleable, conductive. Form CATIONS.

36
Q

The properties of nonmetals are…

A

Solid or gas at room temperature, brittle, nonconductive. Form ANIONS.

37
Q

Elements on the periodic table are arranged according to…

A

Atomic number.

38
Q

The Octet Rule

A

Elements usually react in such a ay to attain the electron of the closest noble gas; elements on the right side of the table move “forward”, and elements on the right side of the table move “backwards.” Based on PERIOD.

39
Q

The Octet Rule is very helpful when…

A

Predicting the charges of ions.

40
Q

A mole contains…particles.

A

6.022 x 10^23

Chemistry 1 (3 decks)

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