Single bond, Saturated, Organic

An observable occurrence in nature that appears to always be true, Summary of a large quantity of information gathered from experiments

Metalloids separate the metals from the nonmetals. What else is true about Metalloids?

They have some metal properties, They include Boron (B), Silicon (Si) and Arsenic, They have some nonmetal properties

Nonmetals are poor conductors, what else is true about nonmetals?

Found on the right side of the periodic table, Several are gases at room temperature, Gain electrons during chemical change

The group numbers represent

Valence electrons of the outermost orbit

Aside from being great heat and electricity conductors what else is true about metals?

Lose electrons during chemical change, Found on the left side of the periodic table

What are the proper charges for each subatomic particle?

Protons= +1, Neutrons= 0, Electrons= -1

What is true regarding atoms and their two distinct regions?

Positively charged nucleus, negatively charged orbitals, Uncharged neutrons in the nucleus, Negatively charged electrons are on the orbitals, Positively charged protons are in the nucleus

Select the intensive properties

Yellow #2 pencil, Boiling point, Cold

A pure substance has only one component and can be chemical elements or compound. Examples include

A bottle of water (H2O), An oxygen tank (O2)

Using the element helium on the periodic table, what does the number 4 represent?

Atomic mass, Total mass of neutrons electrons and protons

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MLT CHEM102

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Questions 98

Answers

1
Alkane
Single bond
Double bond
Saturated
Organic
2
Scientific law
An observable occurrence in nature that appears to always be true
Summary of a large quantity of information gathered from experiments
A set of statements or principles devised to explain a group of phenomena
I am the law.
3
Metalloids separate the metals from the nonmetals. What else is true about Metalloids?
They have some metal properties
They include Boron (B), Silicon (Si) and Arsenic
They are all gases at room temperature
They have some nonmetal properties
4
“Litcherally” the only other formula with two Oxygen :)
Carboxylic acids
Ester
Ether
Amide
5
Nonmetals are poor conductors, what else is true about nonmetals?
Found on the right side of the periodic table
Several are gases at room temperature
Lose electrons during chemical change
Gain electrons during chemical change
6
The group numbers represent
Valence electrons of the most complete orbit
Valence electrons of the innermost orbit
Valence electrons of the outermost orbit
The atomic mass
7
These formulas with COOH are examples of
Ketone
Ester
Easter
Carboxylic acids
8
Using the element helium on the periodic table, if 2 represents the number of protons we can assume
Neutrons= 4
Neutrons= 0
Neutrons= 2
Electrons= 4
9
These formulas that contain Nitrogen WITHOUT Oxygen are examples of
Carboxylic acids
Ester
Amide
Amine
10
Studying all chemical elements except for carbon and hydrogen
Organic chemistry
Both inorganic and organic chemistry
None of the above
Inorganic chemistry
11
Nonmetallic elements tend to form
Negatively charged anions
Positively charged cations
12
These formulas with COH are examples of
Aldehyde
Carboxylic acids
Ester
Amide
13
Periodic law: The physical and chemical properties of elements are periodic functions of their atomic mass
True
False
14
Aside from being great heat and electricity conductors what else is true about metals?
Liquid at room temperature
Lose electrons during chemical change
Found on the left side of the periodic table
Gain electrons during chemical change
15
This is the formula for
Aldehyde
Alkynes
Alkanes
Alkenes
16
These formulas that include a Nitrogen and COH are examples of
Amide
Ester
Aldehyde
Carboxylic acids
17
How many periods are there?
8
6
7
4
18
This is the formula for
Alkanes
Alkenes
Alcohols
Ether
19
Preparing a solvent in the lab
Organic chemistry
Physical chemistry
Biochemistry
Inorganic chemistry
20
Group B elements
All nonmetals
Representative metals
Metalloids
Transition metals
21
Metallic and transitional elements tend to form
Negatively charged anions
Positively charged cations
22
What are the proper charges for each subatomic particle?
Protons= +2, Neutrons= +1, Electrons= 0
Protons= +2, Neutrons= +1, Electrons= -2
Protons= +1, Neutrons= 0, Electrons= -1
Protons= +1, Neutrons= 1, Electrons= -1
23
The elements of the periodic table can be classified as metal, metalloid, or nonmetals
True
False
24
Horizontal rows of the periodic table are
Diagonal
Periods
Groups
Families
25
What is true regarding atoms and their two distinct regions?
Positively charged nucleus, negatively charged orbitals
Uncharged neutrons in the nucleus
Negatively charged electrons are on the orbitals
Positively charged protons are in the nucleus
26
Group A elements
All nonmetals
Representative elements
All metals
Transition elements
27
Polyatomic ions end in
-ide (smaller)
-ite (smaller)
-ate (bigger)
-ite (bigger)
28
Some diatomic molecules include
H, N, O, F, Cr, B
He, O, F, Br, Cl,
H2, N2, O2, F2, Cl2, Br2, I2
NaCl, Fe, Cu2+
29
These TRIPLE bonded carbons are
Alcohols
Alkynes
Alkanes
Alkenes
30
Vertical columns of the periodic table are
Perpendicular
Groups or families
Periods
Horizontal
31
Select the intensive properties
Twenty pencils
Yellow #2 pencil
Boiling point
Cold
32
The smallest unit that retains chemical properties is the atom. What are the primary subatomic particles?
Electron
Proton
Electric
Neutron
33
Extensive properties are dependent on the amount of material. Select the extensive properties
Blue
Hard
Deflated
Heavy
34
Elements whose atoms have an incomplete d sub-shell
Representative metals
Noble gases
Transition metals
Metallics
35
Stock system uses Roman numerals while common nomenclature uses -ic, -ous
True
False
36
In the transitional metal common nomenclature system what should be the ending for the higher charged element?
-ous
-ium
-ic
-al
37
A pure substance has only one component and can be chemical elements or compound. Examples include
A bottle of water (H2O)
Salt water (NaCl and H20)
An oxygen tank (O2)
Chocolate chip cookie dough
38
Periods represent
Valence electrons
The number of orbital rings
The family
The type of metal
39
The minimum energy required to completely remove an electron from an atom
Ionization energy
Electron affinity
Electronegativity
40
Engineering a rocket using semiconductors and high-temperature ceramics
Physical chemistry
Analytical chemistry
Organic chemistry
Inorganic chemistry
41
Atomic size increases from
Bottom to top
Left to right
Top to bottom
42
A property that does not change as the amount of matter changes. It is independent of of the quantity
Extension
Extrinsic
Intensive
Insensitive
43
Elements usually react in such a way as to attain the electron configuration of the noble gases closest to them
Elemenop
Periodic rule
Atomic law
Octet rule
44
Performing a toxicology report to detect the amount of snake venom
Biochemistry
Physical chemistry
Analytical chemistry
Organic chemistry
45
In the transitional metal stock system how would you write FeCl2
Iron (III) chloride
Iron chloride (III)
Ferrous chloride
Iron(II) chloride
46
If numerous experiments support a hypothesis
A hypothesis is formed
A conclusion is formed
A law is established
A theory is established
47
A measure of the ability of an atom in a chemical compound to attract electron
Electronegativity
Electron affinity
Ionization energy
Electro positivity
48
Using the element helium on the periodic table, what does the number 4 represent?
Number of electrons
Atomic mass
Atomic number
Total mass of neutrons electrons and protons
49
These DOUBLE bonded carbons are examples of
Alkanes
Ether
Alkenes
Alcohols
50
Anions are negatively charged
True
False
51
Developing a drug in a lab using a combination of hydrocarbons
Biochemistry
Inorganic chemistry
Organic chemistry
Both inorganic and organic chemistry
52
Group VIII consists of
Noble gases
Alkali metals
Alkali earth metals
Halogens
53
Bonds that have a transfer of electrons
Ionic
Covalent
54
Explaining the difference between the weight of matter in space versus on earth
Organic chemistry
Physical chemistry
Biochemistry
Analytical chemistry
55
If 4 represents the atomic mass or total sum of each subatomic particle how do we find the # of electrons?
Subtract protons from the atomic number
Subtract protons from the mass number
4-2=2
2x2=4
56
Ionic compounds tend to form between
Metals and metals
Metals and nonmetals
Diatomic molecules
Covalent compounds
57
Two types of mixtures are homogenous and heterogeneous. Which of the following are true?
Heterogenous: the components are uniform
Homogenous: composition is uniform
Homogeneous: composition is not uniform
Heterogeneous: the components are not uniform
58
Studying the glycolysis (breakdown of glucose molecules) and it’s affects on the growth of an organism
Organic chemistry
Biochemistry
Physical chemistry
Inorganic chemistry
59
Using the element helium on the periodic table, what does the number 2 represent?
Number of electrons
Atomic mass
Number of protons
Atomic number
60
Electronegativity of covalent polar bonds
0.5-1.9
<-1
<0.5
>1.9
61
Anything that has mass and volume (takes up space)
Matter
Molecules
Atoms
Gas
62
An atom or molecule which has a different number of protons and electrons and thus a net electrical charge
Isotopes
Compound
Ionic bond
Ion
63
The ability to do work, where work is movement of an object by some force
Energy
Chemical reaction
Caffeine
Physical properties
64
Select all true statements
Saline is heterogeneous
Saline is homogeneous
A baked chocolate cookie is homogeneous
Chocolate chip cookie dough is heterogeneous
65
Aliphatic hydrocarbon
Non aromatic rings
Straight chains, branched chains
Aromatic
Benzene ring
66
The metalloids include Germaine (Ge), Anthony (SB), and teletuby
False
True
67
Treating sources of water by first detecting the quantity of toxins
Biochemistry
Physical chemistry
Organic chemistry
Analytical chemistry
68
The number of protons in the nucleus of an atom of the element
Valence electron
Atomic mass
Atomic nucleus
Atomic number
69
What state of matter has a definite volume but no definite shape?
Gas
Liquid
Solid
70
A valid hypothesis must
Summarize a large quantity of information
Prove your observation to be true
Be supported by extensive experimentation
Be testable and falsifiable
71
A mixture is a combination of two or more pure substances
True
False
72
A positively charged ion
Cation
Anion
Isomer
Isotope
73
an idea or explanation that can be tested through study and experimentation
Educated guess
Theory
Epiphany
Hypothesis
74
The “Z” represents
The atomic number
The element symbol
Add answer
The atomic mass
75
Atoms that have the same number of protons, but different number of neutrons; thus, different atomic mass
Ionic bond
Ion
Compound
Isotopes
76
Elements in which all of the inner shells are complete but the outer shell is incomplete
Metallics
Representative metals
Noble gases
Transition metals
77
Total mass of the protons, neutrons, and electrons in a single atom when at rest
Atomic nucleus
Atoms
Atomic mass
Atomic number
78
The basic structural unit of an element
Nuetron
Matter
Nucleus
Atom
79
Electron configuration describes how electrons are arranged within the atom. Gives an atom specific properties
True
False
80
Monotonic ions end in
-ium (+ charge)
-ic (+)
-ium (- charge)
-ide (-charge)
81
What state of matter has no definite volume and no definite shape?
Liquid
Solid
Gas
82
The periodic table groups the elements according to
Aromatic and non aromatic scents
Alphabetical order
Color and atomic mass
The structure and chemical/physical properties
83
What is the difference between a chemical and physical property?
chemical can only be observed during a chemical reaction
Physical can be observed without changing identity of a substance
Chemical and be observed without changing the identity
84
“X” represents
The atomic number
The number of protons
The atomic mass
The element symbol
85
Unequal sharing of electrons (one side is more negatively charged with electrons)
Ionic bonding
Polar covalent bonding
Diatomic bonding
Unilateral bonding
86
These SINGLE BONDED formulas ending in a single OH are
Carboxylic acid
Aldehydes
Alcohols
Alkenes
87
Covalent bonds
Transfer electrons
NaCl
Share electrons
Are ionic
88
What state of matter has both definite volume and definite shape?
Gas
Solid
Liquid
89
(He) which is at the top of Group VIII has how many valence electrons?
8
3
2
6
90
Electronegativity of covalent bonds
0.5-1.9
<0.5
>1.9
<-1
91
Electronegativity of ionic bonds
>1.9
<0.5
<-1
0.5-1.9
92
Assessing a patient’s SPO2 and administrative oxygen
Analytical chemistry
Physical chemistry
Biochemistry
Organic chemistry
93
“A” represents
The element symbol
The atomic mass
The fighting spirit of the Navy
The atomic number
94
A candidate providing a urine sample for pre employment screening
Physical chemistry
Organic chemistry
Analytical chemistry
Biochemistry
95
In the transitional metal common nomenclature system what should be the ending for the lower charged element?
-ous
-al
-ium
-ic
96
Group 1 is mostly
Alkali earth metals
Halogens
Noble gases
Alkali metals
97
The attractive force between ions resulting in electron transfer
Hydrocarbon bond
Ionic bond
Covalent bond
James Bond
98
What are the two types of physical properties?
Intrinsic
Extensive
Extrinsic
Intensive

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