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Science > Chemistry Exam 2 > Flashcards

Chemistry Exam 2 Flashcards

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1
Q

who was first to use the word “atom”

A

Democritus

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2
Q

who discovered that matter consists on atoms, atoms can’t be created or destroyed, and atoms of elements have the same properties?

A

John Dalton

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3
Q

who discovered electrons?

A

J.J. Thompson

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4
Q

who discovered the nucleus?

A

Ernest Rutherford

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5
Q

who found that electrons orbit the nucleus?

A

Niels Bohr

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6
Q

who found the wave nature of electrons?

A

Louis de Broglie

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7
Q

who discovered the nuetron?

A

James Chadwick

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8
Q

modern structure of an atom

A

Electron Cloud Model

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9
Q

what do you add to get the atomic mass of an element?

A

protons and nuetrons

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10
Q

where are the protons in an atom?

A

nucleus

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11
Q

where are the neutrons in an atom?

A

nucleus

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12
Q

where are the electrons in an atom?

A

electron cloud

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13
Q

what charge does the proton have?

A

positive

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14
Q

what charge does the neutron have?

A

nuetral

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15
Q

what charge does the electron have?

A

negative

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16
Q

which particles in an atom have mass?

A

protons and neutrons

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17
Q

what are ions? how do they form?

A

atoms that gain electrons (nonmetals) or lose electrons (metals)

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18
Q

what is an atom?

A

smallest piece of matter that still has properties of the element

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19
Q

what is an element?

A

matter that is composed of one type of atom

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20
Q

how do you calculate the charge of an atom or ion?

A

protons - electrons or compare protons and electrons

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21
Q

atomic number=

A

protons and electrons

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22
Q

what are valence electrons?

A

outer energy level electrons

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23
Q

how many electrons fit in the first energy level?

A

2

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24
Q

how many electrons fit in the second and third energy levels?

A

8

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25
Q

what are the columns on the periodic table?

A

groups or families

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26
Q

how do the elements within a column compare?

A

have similar chemical and physical properties

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27
Q

what are the rows on the periodic table?

A

periods

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28
Q

how do elements within a row compare?

A

they don’t have much in common, range from metals to nonmetals (left to right)

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29
Q

what are metals?

A

elements with 1,2, or 3 valence electrons

30
Q

where are metals located on the periodic table?

A

left side of the periodic table

31
Q

what are the physical properties of metals?

A

conduct heat and electricity, malleable, ductile, shiny luster

32
Q

what does ductile mean?

A

can be drawn/pulled into wires

33
Q

what does malleable mean?

A

can be hammered into sheets

34
Q

what are the alkali metals?

A

Li, Na, K, Rb, Cs, Fr

35
Q

where are alkali metals found on the periodic table?

A

group 1

36
Q

what are the alkaline earth metals?

A

Be, Mg, Ca, Sr, Ba, Ra

37
Q

where are the alkaline earth metals found on the periodic table?

A

group 2

38
Q

what are nonmetals?

A

elements with 5, 6, 7, or 8 valence electrons

39
Q

where are nonmetals found?

A

right side of the periodic table

40
Q

what are the properties of nonmetals?

A

bad conductors, dull, not malleable or ductile

41
Q

what does brittle mean?

A

if hit with a hammer it would fall apart or crumble

42
Q

what is the only nonmetal on the left side of the periodic table?

A

Hydrogen

43
Q

what are halogens?

A

F, Cl, Br, I, At

44
Q

where are halogens located on the periodic table?

A

group 17

45
Q

what are the noble gasses?

A

He, Ne, Ar, Kr, Xe, Rn

46
Q

where are the noble gasses located on the periodic table?

A

group 18

47
Q

what is chemical bonding?

A

2 or more atoms combine to make a new substance with different properties

48
Q

what part of an atom is involved in chemical bonding?

A

electrons

49
Q

what is the purpose of chemical bonding?

A

to have a full outer ring

50
Q

what are the two types of chemical bonding?

A

ionic and covalent

51
Q

what is ionic bonding?

A

two or more ions combine to form a neutral compound, (metals give up electrons, nonmetals take electrons)

52
Q

between which two types of elements does ionic bonding typically occur?

A

metals and nonmetals

53
Q

why do metals typically give up electrons?

A

they have few electrons in the outer ring

54
Q

why do nonmetals typically take in electrons?

A

almost full outer rings

55
Q

what is covalent bonding?

A

2 or more atoms share electrons

56
Q

how is covalent bonding different from ionic bonding?

A

covalent = sharing electrons
ionic = give and take electrons

57
Q

between what types of atoms does covalent bonding occur?

A

nonmetals

58
Q

what is the difference between a single, double, and triple bond?

A

single = two shared electrons
double = four shared electrons
triple = six shared electrons

59
Q

what are the reactants?

A

elements/compounds before reaction

60
Q

where are reactants found?

A

left side

61
Q

what are the products?

A

elements/compounds after reaction

62
Q

where are products found?

A

right side

63
Q

what are subscripts and what do they tell you?

A

small numbers to the right, tells how many you have

64
Q

what are coefficients and what do they tell you?

A

big number to the left of each compound/element, tells how many molecules you have

65
Q

what does the law of conservation of mass say?

A

mass of all reactants must equal the mass of all products

66
Q

what is an acid?

A

substance that produces hydrogen ions
pH = 0-6

67
Q

what is a base?

A

substance that produces hydroxide
pH = 8-14

68
Q

what are compounds?

A

2 or more substances chemically combined

69
Q

what are mixtures?

A

2 or more substances physically combined

70
Q

what is the difference between homogeneous and heterogeneous?

A

homo = substance looks the same
hetero = different materials can be easily seen

71
Q

3 examples of heterogeneous mixtures

A
  • pizza
  • fruit salad
  • trail mix
72
Q

3 examples of homogeneous mixtures

A
  • salt water
  • lemonade
  • steel

Science (3 decks)

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