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Sophomore Midterms > Chemistry midterm > Flashcards

Chemistry midterm Flashcards

0
Q

a variable whose variation does not depend on that of another

A

independent variable

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1
Q

a theory or law before it has become well established; a tentative explanation for an observation or a scientific notation that can be tested by further investigation

A

hypothesis

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2
Q

a variable whose value depends on that of another

A

dependent variable

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3
Q

a variable that is constant and unchanged in an experiment

A

control

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4
Q

What is the difference between a theory and a scienfitfic law?

A

a theory is a proposed explanation or observation. it presents a model of the way nature works and predicts behavior that extends well beyond the observations and laws from which it was formed. And on the other hand a scientific law is a statement that summarizes past observations and predicts the future ones. It is usually formulated from a series of related observations.

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5
Q

the way that scientists learn about the natural world. It involves observations, laws, hypotheses, theories, and experimentation

A

scientific method

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6
Q

SI units: time

A

second

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7
Q

SI units: length

A

meter

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8
Q

SI units: Mass

A

kilograms

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9
Q

SI units: temperature

A

Kelvin

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10
Q

SI units: volume

A

Liter

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11
Q

Si units: density

A

kilograms

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12
Q

is how close a result comes to the true value.

A

accuracy

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13
Q

refers to how well experimental data and values agree each other in multiple tests

A

precise

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14
Q

what is the density formula?

A

density= mass/volume (d=m/v)

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15
Q

a pieve of metal has a density of 13.1 g/mL. If you have a sample with amass of 18,5 g, what is its volume?

A

1.41 mL

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16
Q

if you have an object t hat has a mass of 35g and a volume of 7mL, what is density?

A

5 g/mL

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17
Q

what is the mass of a piece of wood that has a volume of 6.9 mL and a density of 0.56 g/mL?

A

3.9g

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18
Q 
the systematic approach used in scientific studies is called \_\_\_\_\_. 
a hypothesis 
b control 
c scientific method 
d variable
A

c scientific method

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19
Q 
evolution is an example of a \_\_\_\_\_ 
a theory
b scientific law 
c control 
d model
A

a theory

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20
Q 
the SI unit of mass is the \_\_\_\_\_ 
a second 
b meter 
c kilogram 
d milliliter
A

kilogram

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21
Q 
the SI unit of time is the \_\_\_\_ 
a second 
b meter 
c kilogram 
d none of above
A

a second

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22
Q 
How many meters are in 540 km? 
a 540000 m 
b 5.4 m 
54 m 
d 0.54 m
A

a 540000m

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23
Q 
how many centimeters are in 35mm? 
a 3.5 cm 
b 350 cm 
c 0.35 cm 
d 3500 cm
A

a 3.5 cm

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24
Q 
what is the scientific notation for 0.0046? 
a 0.46 * 10^4
b 4.6 * 10^3
c 4.6 * 10^-3
d 0.46 * 10^-4
A

c 4.6 * 10^-3

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25
Q 
You are playing darts. All of your darts hit the bulls-eye right in the center. This means you have been 
a precise 
b accurate 
c both precise and accurate 
d neither precise not accurate
A

c both precise and accurate

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26
Q 
You are playing darts. All of your darts hit the wall near each other, away from the bulls-eye. This means you have been 
a precise 
b accurate
c both precise and accurate 
d neither precise nor accurate
A

a precise

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27
Q

put in scientific notation: 25,000,000

A

2.5 * 10^7

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28
Q

put in scientific notation: 0.00634

A

6.34 * 1-^-3

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29
Q

put in scientific notation: 160

A

1.60 * 10^2

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30
Q

put in scientific notation: 0.0000003

A

3.0 * 10^7

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31
Q

a piece of metal has a volume of 45 mL and a density of 2.0 g/mL. What is its mass?

A

90 g

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32
Q

convert: 470 cm= ____ m

A

4.7 m

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33
Q

convert: 8.046 km = _____m

A

8046 m

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34
Q

convert: 7008 mm = _____ m

A

7.008 m

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35
Q

convert: 175 lbs = ____ kg (1kg= 2.2lbs)

A

79.5 kg

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36
Q

kool-aid

  • homogeneous
  • heterogeneous
  • element
  • compound
A

homogeneous

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37
Q

chex mix

  • homogeneous
  • heterogeneous
  • element
  • compound
A

heterogenous

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38
Q

oatmenal raisin cookie dough

  • homogeneous
  • heterogeneous
  • element
  • compound
A

heterogeneous

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39
Q

brownie mix

  • homogeneous
  • heterogeneous
  • element
  • compound
A

homogenous

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40
Q

Calcium oxide (CaO)

  • homogeneous
  • heterogeneous
  • element
  • compound
A

compound

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41
Q

silver (Ag)

  • homogeneous
  • heterogeneous
  • element
  • compound
A

element

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42
Q

sodium hydroxide (NaOH)

  • homogeneous
  • heterogeneous
  • element
  • compound
A

compound

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43
Q

Beryllium (Be)

  • homogeneous
  • heterogeneous
  • element
  • compound
A

element

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44
Q

define: can be determined only by changing the substance. Most commonly, include the reactivity of substance

A

chemical properties

45
Q

define: can be determined without changing a substance. Ex: color density, solubility

A

physicial properties

46
Q

define: changes that create a new subatance. ex: reaction of sodium and chloine to make sodium chloride

A

chemical change

47
Q

define: changes that do not create a new substance. for ex: ripping paper, state changes

A

physical changes

48
Q 
dissolving salt (NaCl) in water 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physicial property

49
Q 
chopping down a tree 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physicial change

50
Q 
sodium has been found to react violently with water 
a chemical change 
b chemical property 
c physical change 
d physical property
A

chemical property

51
Q 
iron rusting in water 
a chemical change 
b chemical property 
c physical change 
d physical property
A

chemical change

52
Q 
mercury is a silvery liquid 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physical proprty

53
Q 
koolaid powder is soluble in water 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physical property

54
Q 
ice melts on a hot day 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physical change

55
Q 
the density of water is 1.0g/mL 
a chemical change 
b chemical property 
c physical change 
d physical property
A

physical property

56
Q

elements on the left side of the periodic table that are often shiny metals that conduct electricity

A

metals

57
Q

elements on the right side of the periodic table that are either noble gases or soft, brittle solids that do not conduct electricity

A

non metals

58
Q

elements with properties intermediate of metals and nonmetals and are found along the atair-step line of the meriodic table

A

metalloids

59
Q

elements that are found in Group 1A. These are very highly reactive metals

A

alkali metals

60
Q

elements that are found in Group 2A. These are also highly reactive

A

alkali earth metals

61
Q

elements found in the middle (short columns) of the periodic table

A

transition metal

62
Q

elements that are found in 7A. they are also very highly reactive

A

halogens

63
Q

nonreactive elements that are found in group 8A (alll the way to the right of the table)

A

noble gases

64
Q

vertical columns of periodic table

A

groups

65
Q

horizontal rows of periodic table

A

periods

66
Q

chemical formula for: Sodium Carbonate

A

NA2CO3

67
Q

chemical formula for : C2P4

A

Carbon Phosphide

68
Q

chemical formula for : Tin (IV) sulfide

A

Sn2S4

69
Q

chemical formula for : Calcium nitrate

A

Ca(NO3)2

70
Q

chemical name for : Cs2Se

A

Cesium Selenide

71
Q 
Beryllium 
atomic mass 
atomic number 
# of protons 
# of neutrons 
# of electrons
A 
9
4
4
5
4
72
Q 
Carbon -12 
atomic mass 
atomic number 
# of protons 
# of neutrons 
# of electrons
A 
12
6
6
6
6
73
Q 
carbon -14 
atomic mass 
atomic numer 
# of protons 
# of neutrons 
# of electros
A 
14
6
6
8
6
74
Q 
argon 
atomic mass 
number 
# protons 
# neutrons 
# electrons
A 
40
18
18
22
18
75
Q 
platium 
atomic mass 
number 
# protons 
# neutrons 
# electron
A 
195
78
78
117
78
76
Q 
Which of the following is an example of a homogeneous mixture? 
a Sodim (Na) 
b sodium chloride (NaCl) 
c sugar dissolved in water 
d chocolate chip cookie dough
A

c sugar dissolved in water

77
Q 
which of the following is an example of an element? 
a Sodium (Na) 
b Sodium chloride (NaCl) 
c Sugar dissolved in water 
d chocolate chip cookie dough
A

a Sodium (Na)

78
Q 
On the periodic table, where are the transitions metals located? 
a left 
b right 
c along the stair-step line 
d in the middle, in the short columns
A

d in the middle in the short columns

79
Q 
on the periodic table, where are the noble gases located? 
a left-most column (Group 1A) 
b right-most column (group 8A) 
c along stair-step line 
d in middle
A

b right most column

80
Q 
what is the atomic number of Tungsten (w)? 
a 74 
b 50
c 88
d 2
A

a 74

81
Q 
how many protons does an atom of Beryllium have? 
a 9 
b 5
c 2
d 4
A

d 4

82
Q 
How many neutrons does an atom of Carbon-12 have? 
a 6
b 7
c 8
d 12
A

a 6

83
Q 
how many electrons does a netral atom of lithium have? 
a 3
b 7
c 10
d 2
A

a 3

84
Q

chemical name for LiNO3 (ionic or covalent)

A

lithium nitrate (ionic)

85
Q

chemical formula : ammonium nitrate (ionic or covalent)

A

(NH4)3N ionic

86
Q

chemcial name : P2S3 (ionic or covalent)

A

diphosphorus trisulfide (covalent)

87
Q

mass # formula

A

mass # = protons + neutrons

88
Q

list at least 2 differences between ionic and covalent bonding.

A

Ionic bonding is 1 non metal + 1 metal.
Covalent bonding is 1 non metal + 1 non metal.
Ionic bonding is when one atom either loses or gains electron.
Covalent bonding is where they share electrons

89
Q

describe the difference in naming ionic and covalent compounds.

A

In the ionic bonding you have to add an -ide to the end of the 2nd word
In the covalent bonding you do that as well, but you also have prefixes

90
Q 
What type of bond is made up of a metal and a nonmetal? 
a ionic 
b metallic 
c molecular 
d network covalent
A

a ionic

91
Q 
What type of bond makes up a very hard solid with atoms connected in all directions? 
a ionic 
b metallic 
molecular covalent 
d network covalent
A

a ionic

92
Q 
What type of bond is in diamond (C(s))?
a ionic 
b metallic 
c molecular covalent 
d network covalent
A

d network covalent

93
Q

What type of bond makes up a substance that is made entirely of nonmetal atoms that does not conduct electricity and is a gas?
a covalent
b ionic

A

a covalent

94
Q 
which of the following substances is an example of an ionic bond? (1 non metal and 1 metal) 
a NaOH
b NaCl 
c MgO 
d All of the above 
e none of the above
A

d all of the above

95
Q 
Which of the following substances is an example of a covalent bond (molecular or network)? 
a H2O 
b CO2 
c SiO2 
d all of the above
A

all fo the above

96
Q 
Which of the following elements has 1 valence electron? 
a boron
b lithium 
c carbon 
d phosphorus
A

b lithium

97
Q 
Which of the following elements has 4 valence electrons? 
a hydrogen 
b silicon 
c neon 
d sulfur
A

b silicon

98
Q 
Which of the following elements is a noble gas and does not bond with other atoms? 
a hydrogen 
b argon 
c oxygen 
d florine
A

b argon

99
Q 
How many valence electrons does iodine have? 
a 4 
b 5 
c 6 
d 7
A

d 7

100
Q 
according to the Octet Rule, how many valence electrons do atoms want to have (with the exception of Hydrogen and Helium)? 
a 5 
b 8
c 18
d 10
A

b 8

101
Q

synthesis general formula:

A

A + B = AB

102
Q

decomposition general formula:

A

AB = A + B

103
Q

single replacement general formula

A

AB + C = A + BC

104
Q

double replacement general formula

A

AB + CD = AD + CB

105
Q

Combustion general formula

A

CH4 + 2O2 = CO2 + 2H2O

106
Q

a form of matter that has definite shape and volume

A

solid

107
Q

a form of metter that flows, has fixed volume, and an indefinite shape

A

liquid

108
Q

a form of matter that take the shape and volume of its container; it has no definite shape or volume

A

gas

109
Q

define: unequal sharing of electrons

A

polar bond

110
Q

define: equal sharing of electrons

A

nonpolar bonds

Sophomore Midterms (7 decks)

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