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CHEMISTRY 107: FUNDAMENTALS > Exam 2 - PREP > Flashcards

Exam 2 - PREP Flashcards

topics: GASES, ATOMS AND ELEMENTS, MOLECULES COMPOUNDS AND NOMENCLATURE

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1
Q

2.1) A _________ is a neutral species that is comprised of two or more atoms that are linked together.

A

Molecule

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2
Q

P2Cl5
sub2
sub5
is a type of Binary covalent compound because both phosphorus and chlorine are nonmetals. By using the rules for naming this compound the name is

A

diphosphorus pentachloride

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3
Q

MgClO3
sub3
is an NONBINARY compound because three elements are present in the compound. In this case, recognize the POLYATOMIC ion ClO3-
sub 3 with 1 negative charge.
ClO3- is bound to a metal. the rule is to _____________
therefore the name is __________.

A

The rule for naming compounds with polyatomic atoms attached is
1. keep the same order
2. use the polyatomic name properly (don’t forget the ate, ite, per, hypo)

the name is
magnesium chlorate

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4
Q

During chemical reactions- metals tend to __________
electrons. nonmetals tend to ________ electrons. Noble gases tend to __________ electrons due to their complete outer energy level.

A

lose electrons (cation),
gain electrons (anions),
neither gain nor loose

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5
Q

Naming compounds by their formulas
Na2S (sub2)
Pb3N2 (sub3sub2)

explain each

A

Both are binary compounds, therefore you must add the ide at suffix to the last element.

Na2S is Sodium sulfide
Lead is a transition metal and REQIURES roman numberals to express the type of charge it has. Cross down method can be done it reverse to find the ORIGINAL charges before they synthesized. Therefore Pb’s charge was 2 and N charge was 3. Nitrogen must have an ide at the end because its binary compound.
Pb3N2 is Lead (III) Nitride

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6
Q

2.1) The rows of the periodic table are called: ___________

A

PeRiods

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7
Q

Whats the formula for potassium Nitrate?
explain

A

Potassium nitrate intells K and Nitrogen polyatomic compound. Therefore the rules is for naming a nonbinary compound must be applied.

KNO3 (sub3)

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8
Q

The _______ ________ is the same for all atoms of an element. While isotopes is a species of an element with different # of neutrons.

A

Atomic number

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9
Q

Name the compound SF6

A

Sulfur hexafluoride

it’s a BINARY compound. keeps the ide.
It’s a covelant compound because both are NONmetals. therefore to write symbols correctly add the “honorifics” numerical prefixes
hexa hepta mono etc
hexa is 6.

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10
Q

because the most active metals react with water to form bases, they’re called ________ metals. As you move to the right of the periodic table, the base forming properties ________ and the __________ properties increase.

A

alkali metals
decreases
acid forming

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11
Q

Whats the formula for Sodium sulfide?

A

Na2S
sodium sulfide is made of sodium Na and Sulfur S. they’re a metal and nonmetal. therefore the naming convention is to use their electric charges and cross or reverse cross method. the cross method will give you the correct numver of atoms.
Original is Na1 S2
cross down Na2S

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12
Q

The elements in the first 2 groups are light metals, the metals toward the center are __________ metals.

A

heavy

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13
Q

Whats the formula for Aluminum Chloride?

A

AlCl3
binary compounds are cross up or cross down method iot cancel the charges. Chlorine is -1 Aluminum is +3 so it has to be AlCl3 to

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14
Q

Periodic table charge patterns start
Grp1 ____
Grp2 ____
Grp3-12____
Grp13_____
Grp14_____
Grp15____
Grp16____
Grp17____
Grp18____

A

1 +1 alkali
2 +2 alkali earth
3-12 varies
13 +3
14 0
15 -3
16 -2
17 -1 halogens
18 0 noble gases

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15
Q

2.1) The columns of the periodic table are called: ____________

A

Groups

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16
Q

In general, on the periodic table:
Metallic properties and acid forming properties are greatest on the _______ side and decrease as you move right.

Nonmetallic properties and base-forming properties are greatest on the _________ side of the table and decrease as you move left.

A

left (group 1 and 2)

right (group 18,27)

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17
Q

GAS PROPERTIES
As the temperature of a gas is increased, its __________ energy is increased. thereby increasing random motion.

A

kintetic

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18
Q

Group 17 on the periodic table is called: _______________

A

halogens or (halides organic chem)

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19
Q

What’s the definition of an acid?

A

“a water solution that has an excess of hydrogen ions”

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20
Q

an acid turns litmus paper pink or red, has a sour taste, and _________ __________ to form ________.

A

neutralizes bases
salts

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21
Q

definition of a metal:
An element whose oxide combines with ______ to form a base; can also refer to an element that readily ______ electrons and becomes a cation.

A

water
loses

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22
Q

Group 1 on the periodic table is called: ________________

A

Alkaline Metals

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23
Q

definition of a nonmetal:
an element whose oxide reacts with _______ to form an acid; can also refer to an element that takes on an ________ and acquires a negative charge anion.

A

water
electron

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24
Q

What group is the Alkaline Earth metals?

A

Group 2

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25
Q

plasma is very hot ionized _______.

A

gases

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26
Q

What group are the halides in?

A

Group 17

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27
Q

a chemical reaction is a __________ _________. the four basic types are combination (synthesis), decomposition (analysis), single replacement or single displacement, and double replacement or double displacement.

A

chemical change or transformation

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28
Q

What group are the noble gasses?

A

Group 18

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29
Q

Ions are defined as,

A

a atom or group of combined atoms that carry one or more electric charges

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30
Q

Name some elements in group 18:

A

Ne (neon)
Rn (Radon)
He (helium)
Og (Ogganeeson)
A (argon)
K (Krypton)

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31
Q

FORMULA WRITING RULES:
Binary compounds containing a metal with only one charge possibility (Li+1) + nonmetal element

Binary compounds containing a metal element that has more than one charge possibily (ie Fe) + nonmetal element

Binary COVALENT compounds containing two nonmetal elements rules….

A

Rule 1. write down the elemental symbols
2. cross subscripts to balance the charges use “Cross down method”
balance charges to make the resulting overall compound neutral
(AlCl3) (metal with 1 charge possible and non metal)

metal with more that one possible example Iron (III) Oxide.

for binary COVALENT (sharing electron) rules are 1. write down the elemental symbol
2. use the prefixes (di,hept,pent,etc) and write the subscript for each element. (ex sulfur hexafluoride bc sulfur is group 16 fluoride 17)

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32
Q

FORMULA WRITING RULES:

NONBINARY compounds ionic compound containing atleast three elements

A
  1. write down the elemental symbols or polyatomic ion formulas (ie NH3 ammonia)
  2. use subscripts to balance the charges of of the ions. include parantheses when necessary for multiple molecules.
    ie ammonium phosphate is (NH4)3PO4
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33
Q

Name the two groups that compose the periodic table:

A

Metals and Non-Metals

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34
Q
A
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35
Q

2.1) True/False: Hydrogen can be a Metal and Non-metal?

A

True

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36
Q

2.1) What are metaloids?

A

any element that’s directly adjacent to the zigzag line. The metaloids are transition metals whose properties are less predictable than other elements.

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37
Q

Definition of Atomic Mass

A

A weighted average of the mass of all the isotopes (species of an atom with varying # of neutrons in the nucleus) naturally occurring.

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38
Q

How do you calculate the Atomic Mass of an element?
Give a formula

A

(Mass of Isotope(a)(Abundance of a) + (Mass of Isotope(b)(Abundance of b) + (Mass of Isotope(c)(Abundance of c) + (Mass of Isotope(d)(Abundance of d)…etc

You take the different known species of an element,
convert the abundance percentage to decimal (multiply by 100)
then multiply the decimal of its abundance together with their mass,
then divide by the number of species you have.

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39
Q

What is the atomic mass calculation based on?

A

Their natural abundance and the mass of each isotope added.

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40
Q

Calculate the Atomic Mass of Hydrogen.
H is point 1.008 amu

1H 99.9885 % abundance (1neutron 1 proton) & 1.0078 amu
2H 0.0114 % abundance (2 neutrons 1 proton) & 2.0141 amu
3H 0.0001 % abundance (3 neutrons 1 proton) & 3.0160 amu

A

Final answer: 1.0079126… rounded it’s 1.008amu

Work:
(0.999885)(1.0078amu) + (0.000114)(2.0141amu) + (.000001)(3.0160amu) =
(1.00768amu) + (0.0002296amu) + (0.000003016amu) =

= 1.0079126…

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41
Q

X , the symbol of an element is determined by Z. Z is the number of _____________.

A

protons

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42
Q

The Mass Number represents _______________ While the
_______________ represents the number of protons in an element. And the Atomic Mass represents the weighted average of the number of naturally occurring _____________.

A

the sum of Protons and Neutrons in an element.
The Atomic Number (Z).
Isotopes

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43
Q

Where is the atomic number located on the periodic table?

A

Each element has their atomic number located in the right corner. ie the 1 for H is in the right corner of the box.

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44
Q

Calculate the Atomic Mass of Oxygen

A
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45
Q

The difference between Atomic Weight and Atomic Mass?

A

Atomic Mass is the calculation of a SINGLE isotope’s mass.
Atomic Weight is the average of all the isotopes and their natural abundance.

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46
Q

The difference between Atomic Mass and Mass Number?

A

Atomic mass is the weighted average of masses of the naturally occuring isotopes of a specifies. It’s the average mass of the atoms of an element.

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47
Q

Alkali metals are __________ reactive.

A

1A Groups of elements that are highly reactive

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48
Q

Akaline Earth metals are __________ reactive.

A

2A Groups of elements that are fairly reactive

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49
Q

What’s an Anion?

A

An electrically negative charged atom

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50
Q

What’s a Cation?

A

An electrically positive charged atom

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51
Q

“Oxygen” Dr. Cotton is refering to

A

O2 (g)

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52
Q

“Oxygen atom” Dr. Cotton is refering to

A

O

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53
Q

“Everything on the periodic table is a _____________ with few exceptions.

A

mono-atomic solid

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54
Q

Write the natural formula and state for the following:
Oxygen
Sulfur
Phosphorus
Mercury
Bromine

A

Oxygen is O2 (gas)
Sulfur is S8 (solid)
Phosphorus is P4 (solid)
Mercury is Hg (liquid)
Bromine is Br2(liquid)

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55
Q

Atomic Number (Z) is

A

The number of protons in an atom’s nucleus.

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56
Q

Define atomic theory

A

a theory stating that all matter is composed of tiny particles called atoms.

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57
Q

From memory, how does group 1-2, and group 13-17 form ions according to Dr. Cotton?

Group 1 +/-?
Group 2 +/-?
Group 13* +/-?
Group 14* +/-?
Group 15 +/-?
Group 16 +/-?
Group 17 +/-?

*state the special cases too

A

By looking at the periodic table and knowing what groups are stable and which are not

Group 1 always froms plus 1 cations +1
Group 2 always forms plus 2 cations +2
Group 13 B/Al forms plus 3 cations* +3
Group 14 Carbon and Silicon does not form (for our purposes)* NEUTRAL STATE (consider it 0 for our purposes right now)
Group 15 forms minus 3 anions -3
Group 16 forms minus 2 anions -2
Group 17 forms minus 1 anions -1

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58
Q

All unpredictable species form __________.
and give an example.

A

cations positive ion
example, IRON Fe can form Fe2+ or Fe3+

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59
Q

NOMENCLATURE: for a ___________ is to have the ions name + “ion”
give an example

A

Predictable Cation.
Naming a positively charged atom (Cation) is the atom name + “ion” a suffix.
example:
Na+ Sodium Ion
Ca+2 Calcium Ion
Mg+2 Magnesium Ion
etc

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60
Q

NOMENCLATURE: for a _______________ naming convention is to use Atom name + Roman Numeral + “ion” in order to let people know which species an atom is.
give an example

A

Unpredictable cations
example Iron is Fe
Fe+2 = Iron(II) Ion
Fe+3 = Iron(III) Ion

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61
Q

NOMENCLATURE: For a ________________ the naming convention is to use the atom root + “ide”
give an example

A

Anion
O2- = Oxide
N3- = Nitride

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62
Q

Carbon is a metal or non-metal?

A

non-metal

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63
Q

Mercury is a metal or non-metal?

A

metal

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64
Q

B, Si, Ge, As, Sb, Te, and At are metals, non metals, or metalloids?

A

metalloids

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65
Q

The ____________ is the number of protons in the nucleus of an atom, and is denoted as Z. The number of protons in the nucleus of an atom is the defining trait of an element: Its value determines the identity of the element.

A

Atomic Number
(def. from ext lesson)

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66
Q

The ____________ the sum of the number of protons and neutrons in an atom, and it is denoted as A (and A = #protons + #neutrons). Atoms of the same element may have different ____________.

A

mass numbers

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67
Q

Atoms of an element with different numbers of neutrons (or different mass numbers) are called _____________. The symbol for an ______________ of an element (X) is written by placing the mass number as a superscript and the atomic number as a subscript to the left of the element symbol as shown below.

A

isotopes

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68
Q

The _______________ of an element is the weighted, average mass of all the isotopes present in a naturally occurring sample of that element.

A

atomic mass

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69
Q

2.2 True of False? the suffix “ide” will always refer to a monatomic anion

A

True

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70
Q

What is the convention for naming Ionic Compounds per Dr. Cotton?
with example

A

Take the Cation name - “Ion” then add the Anion element at the end.
ex. Sodium Chloride
Sodium Ion - Ion + Chloride

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71
Q

How do you name the Ionic Compound Fe3+ and O2-

A

Iron(III) Oxide

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72
Q

How would you right the name of the Ionic Compound Ca and Fl?

A

Ca is a cation(2+) and Fluoride(-) is an anion
CaF2

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73
Q

EXPLAIN Why there are 2 Fluoride atoms in the Ionic Compound CaF2??

A

Ca is a Cation with charge 2+ (group2) and Fluoride is an Anion with charge -1(group17). In order to get an overall neutral charge for the compound the COMBINED CHARGES MUST CANCEL OUT.
therefore, the LCD of 2 and 1 is 2. 2 Fluorine atoms must attach to 1 Ca atom so the charges 2(pos)+2(neg)=0.

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74
Q

What are the 7 strong acids?
HCl
HBr
HI
HNO3
H2SO4
HClO4
HClO3

A

Hydrochloric acid
Hydrobromic acid
Hydroiodic acid
Nitric acid
Sulfuric acid
Perchloric acid
Chrloric acid

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75
Q

What are the individual charges of the Ionic Compound Fe2O3

A

The Ionic Compound is Iron(III) Oxide
Using the cross down method to formulate the compound’s correct number of atoms (as per their charges), the individual charges for Fe was positive 3(per III), the charge for Oxygen is negative 2(group16)

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76
Q

What’s the formula for Oxide?
Why?

A

O2 (O subscript 2)
The reason is being the naming convention is to specify “ide” of a negative Oxygen atom.

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77
Q

Why do we use roman numerals to express the charge number on transition metals?

A

The roman numerals represent the positive charge values of unpredicatable elements. This needs to be specified in roman numbers each time, because the charge number is not predictable when it reacts with different atoms. Unlike other atoms who always react to loose or gain electrons predictably i.e O2 always O2.

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78
Q

List the 4 transition metals that are not written with roman numerals because they develop a predictable cation formula
__________ +1
__________ +2
__________ +2
__________ +2

A

Silver ion Ag+1
Nickel ion Ni+2
Zinc Ion Zn+2
Cadmium ion Cd+2

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79
Q

Write the name for the Formula:
CrCl2
explain the charges.

A

Chromium(II) Chloride

the charges need to be so that the compound is overall neutral compound,
Therefore, Chloride (two atoms of chloride) each with a charge of negative -1 means it’s overall negative charge is -2. Chromium needs to be able to cancel out -2 charge. Therefore, it’s cation charge can be predicted as II. Hence Chromium II.

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80
Q

Name the Compound
Mn2O3
(3 subscript, 2 subscript)

A

Manganese(III) Oxide

3 Oxygen atoms means the total charge is 3(-2) = -6. Because O is in Gr16. Therefore, the Mn needs to be able to cancel out the -6 with +6. The Mn has 2 atoms. 2(3) = 6. Therefore the Cation Mn has a positive charge of 3- (III) must be expressed in roman numerals.

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81
Q

You should always reduce your formulas to the lowest whole number ratio.
Mg2+S-2

What would it reduce to?

A

MgS

divide by 2.

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82
Q

Should you indicate the charges in your answers for products?

A

NEVER. The value for charges of compounds should be understood (implied).

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83
Q

Write the formula of
Lead (IV) Dioxide

A

PbO2
(subscript2)

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84
Q

You use roman numerals for transition metals and _______ transition metals to indicate the charges because they’re unpredictable.

A

post transition metals.

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85
Q

Name
CoN2
(subscript 2)

A

Cobalt (VI) Nitride
N brings a Charge of 3*2=-6 therefore for the net charge of the compound to be neutral you must have +6. 1 cobalt cation must bring +6 charge.

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86
Q

True or False
To indicate a negative charge on Bromine it’s fine to write minus 3.

A

False, write 3 minus.
The number is written first, then the + or -. The opposite of an exponent.
Br3-

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87
Q

True/False Polyatomic ions are molecules (multiple atoms of an element bonded together).

A

True

88
Q

Metalloids

A

Elements that fall along the boundary between the metals and the nonmetals in the periodic table; their properties are intermediate betwen those of metals and those of nonmetals.
example
they are shiny (metals)
and brittle (nonmetals)

89
Q

“_________ tend to loose electrons in chemical reactions. They are found at the left side and center of the periodic table.”

A

Metals

90
Q

“A compound formed from two or more nonmetals. These compounds have distinct molecules as their simplest identifiable units.”

A

Molecular Compound

91
Q

“___________ two or more atoms joined in a specific arrangement by chemical bonds and is the smallest identifiable unit of a __________ compound.”

A

Molecule
Molecular

92
Q

“____________ are Elements that tend to gain electrons in chemical reactions. They are found at the upper right side of the periodic table.”

A

Non metals

93
Q

“___________ ions are ions composed of a group of atoms with an overall charge.”

A

Polyatomic

94
Q

Give an example of a polyatomic ion

A

NO3 (subscript 3)

95
Q

(2.2)
True/False
One can calculate/predict the charges of a Monoatomic ions, while with Polyatomic ions you cannot predict or figure out.

A

True

96
Q

NH4+ and NH3+
subscript 4
subscript 3

A

Ammonium and Ammonia

97
Q

-OH or OH-

A

Hydroxide

98
Q

C2H3O2-
subscript2
subcscript3
subscript2

A

Acetate

99
Q

NO3-
subscript 3

A

Nitrate

100
Q

Nitrate

A

NOH3-

101
Q

SO4-2
subscript 4

A

Sulfate

102
Q

PO43-
subscript 4

A

Phosphate

103
Q

CO32-
subscript3

A

Carbonate

104
Q

NO2-
subscript2

A

Nitrite

105
Q

SO32-
subscript3

A

Sulfite

106
Q

PO33-
subscript3

A

Phosphite

107
Q

ClO3-
subscript3

A

Chlorate

108
Q

ClO2-
subscript2

A

Chlorite

109
Q

ClO4-
subscript 4
ClO-
subscript is 1 (implied)

A

perchlorate

110
Q

ClO-
subscript is 1 (implied)

A

hypochlorite

111
Q

Bro4-
sub4
Bro3-
sub3
Bro2-
sub2
Bro-
sub1implied

A

Peribromate
Bromate
Bromite
Hypobromite

112
Q

IO4-
sub4
IO3-
sub3
IO2-
sub2
IO-
sub1implied

A

Periodate
Iodate
Iodite
hypoiodate

113
Q

prefixes and suffixes
hypo _______

per ________

______ mite

______mate

______ ate

A

below/sub/least

indicates hyper or highest

small tiny

friend, counterpart

passionate/full of

114
Q

Molecular/Covalent compounds have _________ bonds. While Ionic compounds have _________ bonds.

A

Covalent
Ionic

115
Q

Binary compounds = _________ elements

Nonbinary Compounds = _____________ elements

A

two elements for binary

more than 2 elements for nonbinary

116
Q

Ionic compounds contain two elements: one ______ one _______.

A

metal (anion)
nonmetal (cation)

117
Q

if two or more polyatomic ions are needed to balance the charge, ________ are used around the polyatomic ion. For instance, the compound Fe(OH)2 has parentheses around the OH group and a subscript of 2 following. This is because there are two hydroxide ions (OH-) in the formula. Without the __________, we would have FeOH2 which is incorrect.

A

Parentheses

118
Q

There must be three or more elements in the formula in order for a compound to be classified as ____________.

A

nonbinary

119
Q

When naming Nonbinary Ionic Compounds the what do you do step by step?

A

The cation is named first followed by the anion. The word ion is omitted, and use roman numerals to express the charge of a metal that varies.

120
Q

Is Ba(OH)2
a. barium dihydroxide
b. barium hydroxide

A

b. barium hydroxide.

For ionic compounds we don’t use numbered prefixes~

121
Q

The _______ ending on the name of an ion means it is an anion or a negatively charged ion or non-metals. _______ is used as a suffix at the end of the name of an atom when any non-metal is present singly and bears a negative charge.

A

“Ide”
as in Nitride
Oxide
Fluoride
Sulfide
Root + “ide”

122
Q

_____________ are made up of nonmetallic elements or nonmetallic elements and ___________.

A

Molecular Compounds

Metalloids

123
Q

Molecular compounds do not contain ______. They are instead made up of discrete units called molecules.

A

ions

124
Q

A molecule is a neutral species that is made up of two or more _______ that share electrons.

A

atoms

125
Q

Binary, Nonbinary, and acids are the 3 ___________ for compounds.

A

molecular categories

126
Q

Acids are divided into two groups: ______________.

A

binary acids and oxyacids.

127
Q

Is potassium fluoride and sulfur dioxide pairs of binary molecular compounds? Explain why or why not.

A

No, they’re not pairs of molecular compounds because the compounds are ionic. Ionic compounds are only formed by the transfer of electrons between the potassium and fluoride atoms.

128
Q

Acids are -

A

compounds that form H3O+ when reacting with water. Must have an H+ Ion in the molecule it combined with.

129
Q

Is N2O3 a binary molecular compound?
Why or why not?

A

Yes, Dinitrogen trioxide (N2O3) is a binary molecular compound because the elements bonded together with nitrogen dioxide with nitrogen (NO2) oxide (NO)

130
Q

a molecular compound are made from only non-metal elements and metalloids. (past the transition metals). give some examples:

A

CO2
N2O5
H2O
PO3

131
Q

whats the difference between an ionic compound and a molecular compound?

A

Ionic compounds are made from a metal and non metal. Plus, there are polyatomic ions involved form./

132
Q

HCl

A

Hydrochloric acid

133
Q

HBr

A

Hydrobromic acid

134
Q

HI

A

Hydroiodic acid

135
Q

HF

A

Hydrofluoric acid

136
Q

List the 7 strong acids

A

HCl Hydrochloric acid
HBr - HydroBromic acid
HI - HydroIodic acid

137
Q

Which of the following is NOT a molecular compound?

A) GeCl4
B) NH4Br
C) PCl3

A

B) NH4Br8

138
Q

Naming Convention
Ate Ions become ic acids
ite ions become _______ acids

A

“ous” suffix
ex: nitrate = nitric

139
Q

Why isn’t NH4Br a molecular compound?

A

Because NH4Br is ionic. the Cation ammonium does not share its electrons but gains one and therefore its not a moleculre.

140
Q

Whats the formula for bromic acid?

A

HBro3

H+BrO3-
“taking the bromate ion and adding a hydrogen.”

141
Q

HBrO is what acid?

A

hypobromous acid

142
Q

A Molecure is made up of two or more atoms that ________ an electron.

A

share

143
Q

_______ molecular compounds are made up of two nonmetallic elements.

A

binary

144
Q

Binary molecular compounds use numeric prefixes to indicate the numbers of atoms of the two elements that share ___________ with a compound.

A

electrons

145
Q

List the Numeric prefixes up to 10:
1 ______
2 ______
3 ______
4 ______
5 ______
5 _______
6 _______
7 _______
8 _______
9 ______
10 _____

A

mono
di
tri
tetre
penta
hexa
hepta
octa
nona
deca

146
Q

Sulfurous acids would have a different suffix instead of ous. What is the suffix?

A

“ite” based on the naming convention.
“Sulfite” become ous in order to indicate how many hydrogens come about from the reaction.

147
Q

What is the chemical formula for Dihydrogen Phosphite?

A

H2PO3-

148
Q

How do you determine the name of a chemical when given just the formula?

A

1st determine the elements involved using their symbols. Then identify the prefixes and use the numbers that they represent as subscripts in the formula. For example, is PCl5 was given you would see P has no subscript but Cl does.
Therefore the name is Phosphorus “penta”chloride.

149
Q

What’s the chemical formula for
Iron (III) sulfite trihydrate
*trihyrdrate is when you add the dot and put 3molecules of hydrogen in the formula.

A

Fe2(SO3)3 * 3H2O

150
Q

Important exceptions to naming conventions with numeric prefixes are the:
water H2O
NH3 ammonia
PH3 ________

A

phosphine

151
Q

Give the chemical formula or the name for the following

A
152
Q

Which of the following compounds are nonbinary?

A) Acetic acid
B) HCHO, formaldehyde
C) ethanol,C2H5OH
D) All of the above are nonbinary compounds

A

D) all of the above are nonbinary compounds

153
Q

heptahydrate means what?

A

To put a dot and then write the chemical formula 7H2O next to your compound. (basically means add water)

154
Q

(2.4) What is the correct name for H2SO3?

A) hyposulfurous acid
B) sulfurous acid

A

B) Sulfurous acid

155
Q

What is the correct name for SCI4?

A) monosulfur tetrachloride?
B) sulfur chloride
C) sulfur tetrachloride

A

C) sulfur tetrachloride

156
Q

name of the compound
Cl2O7

A

Dichlorine heptoxide

157
Q

again… Whats a binary compound? Give an example:

A

a chemical made of two different elements.
NaCl2 sodium chloride

158
Q

What is the correct formula for hydrosulfuric acid?

A) H2SO4
B) H2S
C) H2SO3
D) H2S(aq)

A

D) H2S(aq)
the aq indicates is important bc its a binary compound.

159
Q

Chemical formula for iodic acid is:

A) HI(aq)
B) HIO3
C) HIO

A

B) HIO3
not a binary so no need for aq

160
Q

Which of the following is an oxyacid?

A) nitrous acid
B) hypochlorous acid
C) carbonic acid
D) All of the above

A

D) All of the above

161
Q

What is the name of the acid that contains the following polyatomic group: BrO4-

A) hydrobromic acid
B) bromous acid
C) perbromic acid

A

C) perbromic acid

162
Q

(2.3HW) Which of the following is a binary ionic compound?

a) NaOH
b) FeCl2
c) CaSO4
d) Br2

A

B) FeCl2

163
Q

What is the change on tin in the following compound?
Sn(SO4)2

A) 0
B) 2+
C) 4+
D) 2-

A

C) 4+

164
Q

What is the formula of the compound formed when oxygen and aluminum combine?

A) Al2O3
B) AlO2
C) AlO

A

A) Al2O3
(cross products, process of elimination bc u know 2 needs to be there)

165
Q

What is the formula of the compound formed when magnesium ions and nitride ions combine?

A) MgN
B) Mg3N
C) Mg3N2

A

C) Mg3N2

166
Q

Which of the following pairs has the correct name for given formula?

A) K2O - dipotassium monoxide
B) PCl3 - phosphorus chloride
C) PbCO3 - lead (II) carbonate

A

C) PbCO3 - lead (II) carbonate

167
Q

What is the correct formula for the compound that forms between calcium ions and hydroxide ions?

A) CaOH2
B) Ca2OH
C) Ca(OH)
D) none of the above

A

D) none of the above

168
Q

What is the correct formula for barium hypochlorite?

A) Ba(ClO)2
B) Ba(ClO)
C) Ba(ClO3)2

A

A) Ba(ClO)2

169
Q

The chemical formula for manganese (II) oxide is:

A) Mn2O3
B) Mn3O2
C) Mn3O

A

A) Mn2O3

170
Q

Which of the compounds below is not a nonbinary ionic compound?

A) AgNO3
B) NH4Cl
C) CaCO3
D) All of the above are nonbinary ionic compounds!

A

D) All of the above are nonbinary ionic compounds

171
Q

What is the name of the following compound
NaHSO4?

A

A) sodium hydrogen sulfate
B) sodium hydrosulfate
C) sodium hydrogen sulfite
D) sodium sulfate

172
Q

What statements are true?

1) Bromine is more likely to form a cation than an anion
2) Be is more likely to form a cation than anion
3) For a particular element, a cation will have more electrons that an anion
4) In case of the main group elements, their atoms gain or lose electrons in order to have the same number of electrons as their nearest noble gas

A

2) and 4)

173
Q

Which of the following elements is likely to form an anion?

A) H
B) Mg
C) Se
D) Fe

A

C) Se
Selenium

174
Q

The charge on an aluminum ion having 10 electrons is:

A) 3+
B) 3-
C) 2+
D) 2-

A

A) 3+

175
Q

When tellurium forms an ion which of the following would be the likely ion that would form?

A) Te4-
B) Te6+
C) Te2-
D) none of the above

A

C) Te2-

176
Q

If an atom of bromine gains electrons so that it has a total of 36 electrons, what is the charge on the ion that is formed?

A) 1
B) 1-
C)0
D) none of the above

A

B) 1-

177
Q

Identify the metal that is likely to have variable charges.

A) Zinc
B) Copper
C) Aluminum
D) Barium

A

B) Copper

178
Q

Which of the following is a polyatomic ion?

A) NO2
B) SO3
C) NH4+
sub4
D) Pb4+

A

C) NH4+

179
Q

Select all the statements that are correct?
1) the formula for the hydrogen carbonate ion is HCO32
sub 3
2)The name of the O2- formula is oxide ion
3) The formula of the Mercury (I) ion is Hg+
4) The nitrate ion is an oxyanion

A

2) the name of the O2 formula is oxide ion
4) The nitrate ion is an oxyanion

180
Q

What is the name of the following ion: HSO4-
sub4

A) hydrosulfate ion
B) hydrosulfite ion
C) hydrogen sulfate ion
D) hydrogen sulfite ion

A

C) hydrogen sulfate ion

181
Q

Which of the following is written correctly as the name of the following ion: CO2+

A) copper Ion
B) Cobalt ion
C) Copper (II) ion
D) Cobalt (II) ion

A

D) Cobalt (II) ion

182
Q

Which of the following, if any, is a binary ionic compound?

A) F2
B) KOH
C) AgCl
D) NaClO

A

C) AgCl

183
Q

What is the charge on lead in PbSO4?

A

2+

184
Q

Predict the charge on the silver in the following compound:
Ag2CrO4

A)1+
B)2+
C)0

A

A) 1+

185
Q

Which of the following pairs has the correct formula-name match?

A) K2O
B) CuCO3
D) AgNO3

A

B) CuCO3- Copper (II) carbonate

186
Q

What is the correct formula for the compound that forms from the combination of aluminum and oxygen?
A) Al2O3
B)AlO
C)AlO2

A

A)Al2O3

187
Q

What is the correct formula for the compound that forms between lithium ions and hydroxide ions?

A) LiOH2
B) LiOH
C) Li(OH)2
D) none of the above

A

B) LiOH

188
Q

Give the correct name for the compound with the following formula: PbCO3

A)lead carbonate
B) lead II carbonate

A

B) lead II carbonate

189
Q

What is the correct formula for barium hypochlorite?

A

Ba(ClO2)

190
Q

What is the correct name for SCl4?

A) monosulfur tetrachloride
B)sulfur tetrachloride
C) tetrasulfur chloride

A

B) sulfur tetrachloride

191
Q

The chemical formula for manganese (III) oxide is
‘
A) Mn2O3
B) Mn3O2
C) Mn3O

A

A) Mn2O3

192
Q

Consider an atom of an element X, if this atom gain three electron, which of the statements below would most likely be true for this element?

A) The element is a metal and it forms a cation with a 3+ charge.

B) The element is a nonmetal and it forms an anion with a 3 -charge

C) The element is a metal and it forms an ion with a 3 charge

A

B) The element is a nonmetal and it forms an anion with a 3-charge

193
Q

Which of the following elements is likely to form a cation?

A) lithium
B) tellurium
C) iodine
D) argon

A

A) litium because its inn Group 1 where 1 gains.

194
Q

How many electrons must a strontium atom gain or lose to form the strontium ion?

A) lose 5
B) gain 2
C) lose 2

A

C) lose 2

195
Q

What is the charge on an aluminum ion that has 10 electrons?

A

3+

196
Q

When Tellurium forms an ion which of the following would be the likely formula for the ion?

A) Te4-
B) Te6+
C) Te2-

A

C) Te2-

197
Q

If radium were to form an ion, what is the common charge that it is likely to have?

A) 2+
B) 2-

A

A) 2+

198
Q

When iodine forms an ion, how many electrons do you expect the ion to have?

A)52
B)53
C)54

A

C)54

199
Q

Which of the following is a polyatomic ion?
A) N2
B)Hg2 2+
sub2 charge 2+
C) NH3

A

C) NH3

200
Q

What is the name of the following ion: Pb4+?

A

Lead (V) ion

201
Q

What is the name of the following ion
N3-

A

Nitride Ion

202
Q

Which is the correct formula for the carbonate ion?

A)CO3-
B) CO3 2-
sub 3 charge -2

A

B) CO3 2-

202
Q
A
203
Q

Choose the correct statement as True or False.

1) The cation that forms from calcium ion needs a roman numeral in the name so that the reader knows what is the charge on the ion

2) The cation that forms from calcium ion does not need a roman numeral in the name because there is only one possible cation charge variation

3) Since calcium is in group two of the periodic table, its charge can not be predicted.

4) since calcium is in group 2 of the periodic table, its charge cannot be predicted.

A

2,3,4 are true

203
Q
A
204
Q

Which of the following elements exist as a diatomic molecule?

A) Sulfur
B) Hydrogen
C)Neon

A

B) Hydrogen

204
Q

Name some elements in group 18:

A

Ne (neon)
Rn (Radon)
He (helium)
Og (Ogganeeson)
A (argon)
K (Krypton)

205
Q

Which of the following properties is true for metals?

A) shiny
B) electroconductive
C) malleable
D) brittle
E) A-C

A

E) A-C

206
Q

What is the other name for group 2?

A

Alkaline earth metals

207
Q

What is the average atomic mass of chlorine if the mass of one isotope is 34.97 amu and has a percent abundance of 75.77%. The other isotope has a mass of 36.97 amu and has a percent abundance of 24.23%.

A

35.45 amu

208
Q

Which of the following elements are main group elements?

A) Selenium and Iron
B) Lithium and Lead
C) Silver and Tin

A

B) Lithium and Lead

209
Q

Name 5 transition metals

A

Ti - titanium
V vanadium
Cr chronium
Mn Manganese
Fe Iron
Co Cobalt
Ni Nickel

210
Q

True or False?

1) Silicon and arsenic are shiny but brittle

2) selenium is a nonmetal

3) iron and silver are transition metals

4) Gold and lead are post transition metals

A

1,2,3 are true

211
Q

Name 5 Metalloids

A

Boron B
Silicon Si
Arsenic As
Tellurium Te
Astatine At
Germanium Ge
Antimony Sb
(these are all the metalloids)

212
Q
A

CHEMISTRY 107: FUNDAMENTALS (5 decks)

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