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CHEMISTRY > CH 1A > Flashcards

CH 1A Flashcards

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1
Q

describe two central ideas of chemistry

A
  1. Matter is made of particles
  2. the structure of these particles determines the properties of matter
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2
Q

Differences in the properties of these metal arise from what differences?

A

differences in the structure of their particles

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3
Q

What are the three classifications of solid matter?

A
  1. energy too low to overcome forces
  2. tightly packed
  3. fixed in place
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4
Q

What are the three classifications of liquid matter?

A
  1. energy sufficient to overcome some forces
  2. closely packed
  3. can move
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5
Q

What are the three classifications of gaseous matter?

A
  1. energy sufficient to overcome some forces
  2. closely packed
  3. can move
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6
Q

what are the three classifications of gaseous matter?

A
  1. energy sufficient to overcome all forces
  2. widely spaced
  3. freely move
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7
Q

What particles make up matter?

A

atoms

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8
Q

what are atoms?

A

smallest basic particle

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9
Q

How many different types of particles are there?

A

118 (91 form naturally)

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10
Q

what are the three fundamental particles of matter?

A
  1. individual atoms
  2. molecules
  3. repeating unit of atoms
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11
Q

give an example of individual atoms?

A

Helium (He)

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12
Q

what is a molecule?

A

atoms bonded together in specific geometrical arrangements

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13
Q

give an example of a molecule

A

Ozone O3, Hydrogen Peroxide (H2O2)

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14
Q

what are repeating units of atoms

A

repeating units of atoms are the consistent, repeating arrangement of atoms in a crystalline or structured form.

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15
Q

give an example of repeating units of atoms

A

Sodium chloride (NaCl

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16
Q

what is the difference between repeating units of atoms and molecules?

A

Repeating units of atoms refer to the pattern or arrangement of atoms in a material, particularly in solid forms.
Repeating units of molecules refer to the individual molecular units or monomers that repeat to form larger molecules like polymers.

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17
Q

What is a pure substance?

A

a substance that contains one type of particle

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18
Q

What are two types of pure substances?

A

elements and compounds

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19
Q

What is an element?

A

a pure substance that can’t chemically break down into simpler substances

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20
Q

What is a compound?

A

A pure substance composed of two or more elements bonded together in fixed definite proportions. (more than one type of atom bonded together)

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21
Q

Can a compound be broken down?

A

Yes, compounds can be broken down into elements by a chemical reaction

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22
Q

Give an example of compounds

A

Sodium chloride (NaCl)

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23
Q

what is matter that isn’t made up of one particle?

A

Mixtures

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24
Q

what are mixtures?

A

two or more pure substances blended together in proportions that can vary

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25
Q

what are two types of mixtures?

A

heterogeneous and homogeneous mixtures

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26
Q

what are heterogeneous mixtures

A

mixings that are NOT uniform such that the composition isn’t uniform.

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27
Q

give an example of a heterogeneous mixture

A

sand, cereal in milk, oil and water,

28
Q

what are homogeneous mixtures

A

mixings that ARE uniform such that the composition is the same throughout

29
Q

what are examples of homogenous mixtures

A

Vega’s drink, air, wine, coffee

30
Q

How do we know that matter is made of particles?

A

experimental evidence

31
Q

How do we know that matter is made of particles?

A

Experimental evidence

32
Q

Law of conservation of mass

A

mass of reactants equals the mass of the products for a chemical reaction

33
Q

law of definite proportions

A

In any given chemical compound, the elements are always combined in the same proportion by mass.

34
Q

law of multiple proportions

A

When two elements form more than one compound, the different masses of one element that combine with a fixed mass of the other element are in a ratio of small whole numbers.

35
Q

Lavoisier discovered . . .

A

the law of conservation of mass

36
Q

how did Lavoisier discover the law of conservation of mass

A

by inventing balances, allowing him to weigh the reactions before and afterwards. Shows that the mass was conserved

37
Q

Does the mass of reactants = the mass of products

A

Yes

38
Q

give an example of mass of reactant = mass of products

A

2HgO–> 2Hg + O2

39
Q

what are the four points of Dalton’s atomic theory?

A
  1. each element is composed of tiny indestructible particles called atoms
  2. all atoms of a given element have the same mass and properties; these distinguish them from other elements.
  3. Atoms combine in simple, whole-number ratios to from compounds
  4. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way they are bound together with other atoms.
40
Q

Key characteristics of the scientific method are

A

observations
formulation of hypotheses
experimentation
formulation of laws and theories

41
Q

A hypothesis is a

A

interpretation or explanation of the observations

42
Q

A scientific law

A

is a brief statement that summarizes past observations and predicts future ones. describes patterns

43
Q

Name a scientific law

A

law of conservation of mass

44
Q

A scientific theory is

A

formed from a well-established hypothesis or set of hypotheses. A theory tries to explain why a natural phenomenon happens. (greatest degree of certainty in science)

45
Q

name a scientific theory

A

dalton’s atomic theory

46
Q

in science, a theory is

A

what scientist are MOST CERTAIN about

47
Q

Atoms are made up of what three subatomic particles

A

protons, neutrons, and electrons

48
Q

What is the mass of a proton

A

1.67262 x 10^-27

49
Q

What is the mass of a neutron

A

1.67262 x 10^-27

50
Q

what is the mass of a electron

A

0.00091x10^-27

51
Q

A proton’s charge is

A

1+

52
Q

A neutron’s charge is

A

0

53
Q

An electron’s charge is

A

-1

54
Q

How are atoms arranged?

A

An atom is spherical, composed of a positively charged central nucleus surrounded by one or more negatively charged electrons

55
Q

atomic nucleus consists of

A

protons and neutrons

56
Q

Describe Rutherford’s gold foil experiment

A

He took a gold foil and shot alpha particles through the foil. The alpha particles, upon shooting through, ended up passing through with little deflection. But a small fraction was very strongly deflected, due to encountering something very massive. Suggesting that there was a very small and concentrated volume of protons and neutrons.

57
Q

What was the predicted result of the rutherford’s experiment

A

plum-pudding mode, where the particles are distributed evenly throughout

58
Q

What was the actual result of rutherford’s experiment

A

nuclear model, where the protons and neutrons are centered in a small area

59
Q

What was the conclusion of rutherford’s experiment

A

most of the atom is empty space with its mass largely concentrated in a tiny central core (nucleus)

60
Q

atomic number is

A

the number of protons in an atom

61
Q

mass number

A

the sum of the number of protons and neutrons in an atom

62
Q

ion

A

an atom with a net charge due to loss or gain of electrons

63
Q

isotopes

A

atoms with the same number of protons but different numbers of neutrons

64
Q

mass number is located

A

on the top left of the chemical symbol

65
Q

atomic number is located

A

on the bottom left of the chemical number

CHEMISTRY (2 decks)

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