Chapter 2: The Components of Matter Flashcards

1
Q

Element vs Compound

A

An element is composed of only one type of atom and can’t be broken down into a similar chemical substance by physical or chemical means.
A compound is composed of two or more elements chemical combined.

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2
Q

Define mixture

A

Two or more elements and/or compounds, physically intermingled.

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3
Q

Define a homogenous mixture

A

You can’t pick out components of a homogenous mixture or use simple mechanic means to separate them
Example: air, sugar water, rain water, vodka, vinegar, dishing detergent

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4
Q

Define a heterogeneous mixture

A

A mixture where the components of the mixture are not uniform or have localized regions with different properties.
Example: Chicken soup, cereal, blood, soil, pizza

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5
Q

Explain Law of Mass Conservation

A

The total mass of a substance does not change during a chemical reaction.

MATTER CANNOT BE CREATED OR DESTROYED

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6
Q

Explain Law of Definite/Constant Composition

A

No matter the source, a pure compound is composed of the same elements in the same parts (fraction) by mass

MASS FRACTION IS FIXED NO MATTER WHAT THE SIZE OF THE SAMPLE

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7
Q

Explain Law of Multiple Proportions

A

If element A and B react to form two compounds, the different mass of B that combines with the fixed mass of A can be expressed as a ratio of small whole numbers.

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8
Q

14.35g of kaolinitie contains 8.009g oxygen what is the mass percent of oxygen in this sample? What Law is this an example of?

A

(8.009g/14.35g) x 100 = 55.81%

Law of Constant Proportions

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9
Q
Which pair of substances could be used to illustrate the law of multiple proportions?
A. SO2,H2O
B. SO, SO2
C. H2O, O2
D. CH4, C6H12O6
E. NaCl, KCl
A

B. SO, SO2

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10
Q

What did Millikan discover and what was the experiment?

A

Charge of an electron; Oil Drop

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11
Q

What did JJ Thomas discover and what was his experiment?

A

An atom is composed of smaller particals;Used magnetic and electric fields to measure mass-to-charge ratio of cathode ray particles.

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12
Q

What did Rutherford discover and what was his experiment?

A

Most of atom’s empty space is located in the nucleus, which has a ver small volume/dense partial within the atom; gold foil experiment

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13
Q

Define an Isotope

A

atoms of the element with the same number of protons, but different number of neutrons.

CHANGE IN MASS NUMBER

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14
Q

What is the name of group 1A on the periodic table?

A

Alkaline Metals

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15
Q

What is the name of group 2A on the periodic table?

A

Alkaline Earth Metals

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16
Q

What is the name of group 6A on the periodic table?

A

Chalcogens

17
Q

What is the name of group 7A on the periodic table?

A

Halogens

18
Q

What is the name of group 8A on the periodic table?

A

Nobel/Rare Gases

19
Q

What is in an ionic compound?

A

Metal and Non-Metal

20
Q

What is the name of the binary compound CrCl3?

A

Chromium (III) chloride

21
Q

What is in a molecular compound?

A

Non-Metal and Non-Metal

22
Q

Name the seven elements that occur naturally as molecules containing two atoms?

A

Hydrogen (H2), Nitrogen(N2), Oxygen(O2), Fluorine(F2), Chlorine(Cl2), Bromine(Br2), Iodine(I2)

23
Q

Name the prefix for 1.

A

mono-

24
Q

Name the prefix for 2.

A

di-

25
Q

Name the prefix for 3.

A

tri-

26
Q

Name the prefix for 4.

A

tetra-

27
Q

Name the prefix for 5.

A

penta-

28
Q

Name the prefix for 6.

A

hexa-

29
Q

Name the prefix for 7.

A

hepta-

30
Q

Name the prefix for 8.

A

octa-

31
Q

Name the prefix for 9.

A

nona-

32
Q

Name the prefix for 10.

A

deca-

33
Q

Define a molecular formula.

A

Give the exact number of each element in a compound.

Example - Glucose: C6H12O6

34
Q

Define empirical formula.

A

Gives the lowest whole-number ratio of atoms of each element in a compound.
Example - Glucose: C1H2O1

35
Q

What is the name of the compound S2F4?

A

disulfur tetrafluoride

36
Q

Define molecular mass.

A

Sum of atomic masses.