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Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

The smallest particle of an element that retains its identity in chemical reaction.

A

atom

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2
Q

Who first proposed the idea of the atom and called them atoms

A

Democritus

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3
Q

Atoms were uniform, solid, hair, incompressible, and indestructible
They moved in infinite number through space until stopped
The properties of matter were determined by differences in atomic shape and size.

A

Democritus’ ideas of an atom

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4
Q

Who observed that the mass of reactants in the container before a chemical reaction was equal to the mass of the products after the reaction. This became known as the law of conservation of mass.

A

Antoiine Lavoisier

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5
Q

Joseph Proust observed that the composition of water is always 11 percent hydrogen and 89 percent oxygen by mass. Regardless of the source of the water, it always contains these same percentages of hydrogen and oxygen. This principle is now referred to as the_______.

A

law of definite proportions

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6
Q
  1. All elements are composed of tiny indivisible particles called atoms
  2. Atoms of an element are identical and differ from atoms of other elements
  3. Atoms cannot be created nor destroyed
  4. Compounds are composed of atoms in fixed proportions
A

The 4 parts of Dalton’s Atomic Theory
He basically copied other scientists theories and organized them into the Atomic Theory.

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7
Q

Negatively charged subatomic particles

A

electons

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8
Q

Who first proposed that atoms contained electrons?

A

JJ Thomson

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9
Q

What experimental evidence did JJ Thomson us to prove his theory

A

Used a cothode-ray tube that showed + and - charge

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10
Q

Draw a cathode-ray tube

A
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11
Q

Draw a picture of JJ Thomson’s model of the atom

A
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12
Q

Positively charged subatomic particles

A

Proton

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13
Q

Subatomic particles with no charge but a mass equal to a proton

A

Neutons

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14
Q

What American scientist carried out experiments that allowed him to determine the relative charge and mass of an electrons

A

Ernest Rutherford

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15
Q

Draw a diagram to illustrate what rutherford observed in his experiment

A
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16
Q

From the experiment, Rutherford concluded that an atom is made up mostly of _____ and the mass and positive charge are concentrated in a small region in the center of the atom which is called the _____.

A

Space
Nucleus

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17
Q

How does the size of the nucleus compare to the overall size of the atom? Give an example.

A
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18
Q

Draw a diagram that illustrates Rutherford’s model of the atom

A
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19
Q

What did Niels Bohr propose about the electrons in an atom?

A

They have energy with set energy levels or orbits around the nucleus. Electrons are found in specific circular paths

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20
Q

Draw a picture of Niels Bohr’s model of an atom

A
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21
Q

Energy comes in fixed levels

A

quantized

22
Q

The______of an element is the number of protons in the nucleus of an atom. In a neutral atom of an element, the number of electrons in the atom_____ the number of protons.

A

Atomic number
equals

23
Q

Know what all the symbols on elements mean

A
24
Q

Atoms that have the same number of protons but different number of neutrons

A

isotopes

25
Q

an______is defined as one-twelfth the mass of a carbon-12 atom
Carbon 12 is the _______

A

Atomic Mass Unit
Reference element

26
Q

A weighted average mass of atom in naturally occuring sample of element.

A

Atomic mass/num.

27
Q

Blue number=______ and tells us the number of ______ which determines the _____

A

Atomic number
protons
identity

28
Q

Atomic number=_____=_____

A

protons
electrons

29
Q

Red number=______

A

Mass numbere

30
Q

Mass number=______+______

A

Protons
Neutrons

31
Q

Mass number-Atomic number=

A

neutrons

32
Q

How do you calculate the most common iscotope?

A

Round the mass number
If its in parenthesis there’s only 1 iscotope

33
Q

Steps to calculating atomic mass

A
  1. Change % to decimal
  2. Multiply by mass
  3. Add sum together
34
Q

Atoms whose outer energy levels contain 8 electrons are stable

A

Octet rule

35
Q

electrons have energy because they travel at the speed of light and their________ ________ determines their placement on the rings

A

energy level

36
Q

electrons on the outermost shell and in highest occupied energy level

A

Valence electrons

37
Q

valence electrons largely determine the ______ and _______ properties of an element.

A

chemical and physical

38
Q

How many valence electrons do the transition metals have?

A

2

39
Q

What does the group on the periodic table tell you?

A

The number of valence electrons

40
Q

What does the period of the periodic table tell you?

A

The number of energy levels (rings)

41
Q

Who constructed the first periodic table? and organized the elements in order of increasing atomic mass.

A

Mendeleev

42
Q

The modern periodic table is organized in order of increasing______.

A

atomic number

43
Q

Who was the first person to organize the periodic table in the order of atomic numbers?

A

Henry Mosely

44
Q

Most elements are________.
The 2 elements that are liquids are ______ and ______.
The gaseous elements, except hydrogen, are located in the_____ side of the periodic table.
Elements __, __, and __ and above are synthetic elements.
Synthetic elements are elements that are ___ found in nature.

A

Solids, bromine, mercury, right, 43, 61, 93, not

45
Q

how can you determine whether an element is a metal, nonmetal, or metalloid based on its position on the periodic table?

A

The step stair line seperates the metals on the left from non-metals on the right, elements that straddle the line are called metalloids.

46
Q

solid, good conductors of heat and electricity, ductile, malleable, lustrous.

A

Metals

47
Q

most are gases, not good conductors of heat and electricity, brittle

A

Nonmetals

48
Q

Semiconductors of heat and electricity

A

Metalloid

49
Q

The most well known metalloid is ______.
Elements is groups__, __, and __ through__ are called Representative elements

A

silicon, 1, 2, 13, 18

50
Q

Elements is group__ are called alkali metals
Elements in group__ are called Alkaline-Earth Metals

A

1, 2

51
Q

Elements in group__ are called Halogens or ______.
Elements in group__ are called Noble Gases.

A

17, Salt formers, 18

52
Q

Elements in groups __ through __ are called transition metals.
Elements __ through__ are called lanthanides or _______.
Elements __ through__ are called Actinides

A

3, 12, 57, 70, 89, 102

Chemistry (17 decks)

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