Chemistry Flashcards
1
Q
Finish this sentence: Chemistry helps us…
A
understand the properties and composition of the world around us.
2
Q
What is matter?
A
Anything that has mass and takes up space
3
Q
What is the particle Theory of matter?
A
A model that has been developed to help us understand matter. Helps us visualize how matter behaves and helps to explain why different matter can display different properties
4
Q
What is a model?
A
A scientific way of thinking.
5
Q
What is all matter made up of?
A
All matter is made up tiny particles, either individual atoms, or groups of atoms called molecules.
6
Q
What is in the centre of each atom?
A
the nucleus
7
Q
What is within the nucleus?
A
Within the nucleus there are positively charged particles called protons and particles with no charge called neutrons.
8
Q
What is the nucleus held together by?
A
Strong nuclear force
9
Q
What is orbiting around the nucleus?
A
Negatively charged particles called electrons
10
Q
Are atoms neutral? What does that mean?
A
Yes atoms are neutral. This means that the number of electrons (negatives)must equal the number of protons (positive)
11
Q
What are electrostatic forces?
A
forces that attract negatively charged and positively charged particles to each other.
12
Q
What does electrostatic forces do in an atom?
A
Electrostatic forces keep the electrons orbiting around the positive charges of the nucleus.
13
Q
What defines the type of atom?
A
the number of protons in the nucleus defines the type of atom.
14
Q
How many protons does a gold atom have? How many protons does a silver atom have?
A
gold = 79 protons silver = 47 protons
15
Q
How much heavier are protons and neutrons that electrons?
A
much heavier– 2000 times heavier- most of the weight of an atom is due to nucleus
16
Q
True or false - Are atoms mostly empty space?
A
Yes - There is nothing in between the nucleus and the electrons, which means atoms are mostly empty space.
17
Q
What is absolute zero?
A
-273.15 degrees Celsius also called 0 Kelvins ( O K)
18
Q
What do particles of matter do at a temperature above absolute zero?
A
At temperatures about absolute zero particles of matter are constantly moving even though the human eye cannot see anything move.
19
Q
How does speed affect the temperature of particles?
A
The higher the average speed of particles, the higher the temperature.
20
Q
What is property?
A
Something that describes matter.
21
Q
What does property of matter allow us to identify?
A
Property of matter allows us to identify substances.
22
Q
Name examples of Physical properties.
A
Color, odour, taste, size, shape, boiling point, hardness, malleability, electrical conductivity, magnetism, and density.
23
Q
What is Physical property?
A
Physical property is a characteristic of matter that we can measure.
24
Q
What is Malleability?
A
The ability to be pounded flat.
25
What is the chemical property of a substance?
Chemical property is a characteristic of a substance which describes its potential to undergo a chemical reaction or change.
26
Name some examples of Chemical Properties.
Flammability, Reactivity, Corrosiveness, toxicity
27
Describe Flammability.
ability to burn
28
Describe Reactivity.
ability to react when combined with another substance ( ie, baking soda & vinegar)
29
Describe Corrosiveness.
ability to "eat away" another substance (ie, oxygen causes iron to rust and flake off)
30
Describe Toxicity.
ability to cause damage to living organisms (ie, lead, mercury, chlorine gas)
31
What do you call matter that is composed of only one type of atom?
An element.
32
What is atomic symbol?
1 to 3 letter internationally agreed code for a chemical element.
33
What is the atomic symbol Uuo?
Uuo was discovered in October 2006, by the Flerov Laboratory of Nuclear Reactions in Dubna, Russia. Called element 118, Ununoctium.
34
What were the official names given to the elements 114 & 116 on Thursday May 31, 2012?
114 - Flerovium (fl) 116 Livermorium (Lv)
35
What is the atomic symbol and word origin of Gold?
Au - Latin word aurum meaning 'shining dawn'
36
What is the atomic symbol and word origin of Mercury?
Hg - Greek word hydragyrum meaning 'silver water'
37
What is the atomic symbol and word origin of Chlorine?
Cl - Greek word chloros meaning 'green'
38
What is the atomic symbol and word origin of Neon?
Ne - Greek word neos meaning 'new' or 'different'
39
What is the atomic symbol and place of origin of Europium?
Eu - Europe
40
What is the atomic symbol and place of origin of Francium?
Fr - France
41
What is the atomic symbol and place of origin of Germanium?
Ge - Germanium
42
What is the atomic symbol and place of origin of Berklium?
Bk - Berkeley, California
43
What is the atomic symbol and place of origin of Dubnium?
Db - Dubna, Rusia
44
What is the atomic symbol and Famous scientist for Curium?
Cm - Pierre and Marie Curie (research in radioactivity)
45
What is the atomic symbol and Famous scientist for Einsteinuim?
Es - Albert Einstein
46
What is the atomic symbol and Famous scientist for Nobelium?
No - Alfred Nobel (of Nobel Prize fame)
47
What is the periodic table of elements?
The periodic table of the elements is a way of displaying information about the elements in a table format.
48
Who is usually credited with devising the first periodic table in 1869?
Dmitri Mendeleev is credited with devising the first periodic table. Working independently Lothar Meyer came up with an almost identical table later the same year.
49
What is listed in the box of an element on the periodic table?
Its atomic symbol and atomic number. The elements full name and atomic mas may also be given.
50
What does the entry for the element Calcium look like on the periodic table?
20 Atomic Number: 20
Ca Atomic Symbol: Ca
Calcium Atomic Name: Calcium
40.078 Atomic Mass: 40.078 unified
atomic mass units (u)
Element Classification: Metal
51
What is the atomic mass of an element?
The atomic mass of an element refers to the average mass of an element in unified atomic mass units. Usually given an the bottom of an elements entry in the period table.
52
What is the short form of atomic mass units?
u
53
How does the atomic mass appear on the periodic table?
It appears as a decimal number because it is an average of the masses of the various isotopes of an element.
54
Do Isotopes of an element have the same number of protons?
Yes
55
Do Isotopes have different numbers of neutrons in the nucleus?
Yes. Isotopes of an element have the have number of protons, but different numbers of neutrons in the nucleus.
56
Does the most common isotope of hydrogen have neutrons?
No! the most common isotope of hydrogen has no neutrons at all.
57
How many neutrons does the isotope deuterium and tritium have?
Deuterium has 1 neutron and deuterium has 2.
58
Describe the isotope of hydrogen (4H-7H)
Highly unstable, made in the laboratory, does not occur in nature.
59
How do you find the average number neutrons for an element?
By subtracting the number of protons (atomic number) from the atomic mass.
60
What is the average number of neutrons for calcium?
Calcium has an atomic number of 20 and an atomic mass of 40.078amu. By subtracting 20 from 40(rounded) you get 20 (protons + neurons = atomic mass)
61
Did Mendeleev organize his table to illustrate that chemical properties occurred periodically with increasing mass or decreasing mass?
Increasing mass (called periodic law)
62
How did Mendeleev organize his table?
He began new rows (periods) in his table so that elements with similar properties fell into the same column. His table also contained gaps for new elements not yet discovered.
63
How was Mendeleev able to predict the properties of mising elements?
Based on the properties of the other elements within that column.
64
What are the columns in the periodic table known as?
Groups
65
When was Mendeleev's table rearranged?
During the 1900's discoveries led to new elements and Mendeleev's the table was rearranged to give us the format we use today.
66
According to international chemistry rules, the groups on the periodic table are numbered how?
1 to 18
67
Describe the elements in group "18"
Group 18 is gases that do not readily react with other elements. These gases are know as NOBLE GASES.
68
With the exception of hydrogen, what are the elements on the left side of the periodic table know as?
Metals
69
What are metals?
Metals are solid at room temperature. The exception is Mercury which is liquid. Metals are malleable, and ductile, have a shiny appearance and are good conductors of heat and electricity.
70
What does ductile mean?
Can be stretched out to form a wire.
71
Elements on the right side of the periodic table are know as what? and describe.
Non-metals. They can be solids, liquid or gases and are poor conductors of heat and electricity.
72
What are metalloids?and give examples
Metalloids have some metallic as well non-metallic properties. Examples are Silicon & arsenic
73
What is the D-block on the periodic table?
D-Block is elements in groups 3-12. They are also know as transition elements.
74
What are the two rows placed in a block at the bottom of the periodic table known as?
The Lanthanide series and Actinide series.
75
What is the Lanthanide Series?
The Lanthanide Series is made up fifteen metallic elements with atomic numbers 57- 71, from lanthanum to lutetium. Lanthanide Series can be found naturally on Earth.
76
What are the rare earth elements?
The fifteen lanthanide elements along with the chemically similar elements scandium and yttrium are collectively know as the rare earth elements.
77
Can members of the Lanthanide series be found naturally on Earth?
Yes
78
How is the Actinide series different from the Lanthanide?
All of the Actinide series element are radioactive and some are not found in nature. Some of the elements with higher atomic numbers have only been made in laboratories.
79
What does the size (radius) of an atom do as it moves down a group on the periodic table?
The size of an atom increases as you move down a group.
80
Why do atoms increase in size at the bottom of a group?
Because towards the bottom of a group, elements have more layers of electrons.
81
What does the atomic size of an atom generally do from left to right with a period?
Decreases.
82
Why does the atomic size generally decrease from left to right within a period?
Because as you increase the number of protons, the shell of electrons get pulled tight to the nucleus.
83
What is Electronegativity?
A chemical property that describes the tendency of an atom to attract electrons towards itself.
84
What does Electronegativity do in a group and a period?
Electronegativity usually decreases down each group and increases from left to right across a period.
85
Where are the most electronegative elements found? Why?
The most electronegative elements are found in the upper right hand side of the periodic table. This is because non-metals which have high electronegativity, tend to pull electrons from other atoms. Metals tend to lose electrons.
86
What does electrically charged mean?
Electrically charged means, experience a force when near by other electrically charged matter.
87
What must atoms do to become electrically charged?
Atoms must lose or gain electrons to become electrically charged.
88
What are the two types of electric charges?
Positive charges + & Negative charges -
89
How do Positively charged substances act?
Positively charged substances repel other positively-charged substances and attract negatively-charged substances.
90
True or False? .Elements in group 1 (ie: Li, Na, K) tend to easily lose one electron which gives then +1 charge
True
91
True or False? Elements in group 17 (ie, Cl, Br, I) tend to easily gain one electron which gives them -1 charge.
True
92
When at atom or molecule has more electrons or fewer electrons than the total number of protons(has a positive or negative electrical charge) then it is said to be, what?
Ion
93
What is anion?
When an atom on molecule has more electrons than protons, the result is a negative ion, which is anion.
94
What is Cation?
When an atom or molecule has fewer electrons that protons, then the result is a positive ion which is Cation.
95
Each group in the period table has a specific charge commonly associated with its ions except for which elements?
The exception are the lanthanide and actinide series.
96
What are the specific charge associated with is ions for each group in the period table?
Group 1 = +1 Group 2= +2 Group 13=+3 Group 15= -3 Group 16= -2 Group 17= -1
97
Why does group 18 have a charge of 0?
These elements are very stable and they do not readily gain or lose electrons.
98
What are the 2 changes matter undergoes can undergo every day?
Physical changes or Chemical changes
99
True or False? Can physical changes almost always can be reversed to get back what you originally had before the change took place. Give example for answer
True. Example- When liquid water freezes into ice you still have water, it is just in a different state, it went from a liquid to a solid.
100
What is a phase change
A phase change is a change in state or form in which no new substance is formed.
101
What are some examples of processes in our body that require chemical changes?
Digestion, respiration, thinking are examples of processes in our body that require chemical changes.
102
What is a chemical change or chemical reaction?
A process by which one or more substances are changed into others through chemical means. A chemical change is a change in which at least one new substance is formed.
103
What are some observable changes to tell when a chemical reaction has occurred?
Formation of a gas, a change in color, a change in temperature, the emissions of light, the appearance of a new substance and sometimes a change in the amount of reactants or products.
104
What is a reactant?
A reactant is the substance you begin with
105
What is the product?
The product is the substance you have after the reaction.
106
Many chemical reactions involve a transfer of what?
Transfer of energy. In some cases in may be felt as heat energy and in others it may be seen as light.
107
When a chemical reaction gives off heat and feels hot what it is called?
Exothermic
108
When a chemical reaction requires heat, and it feels cold?
Endothermic
109
What happening when you crack a glow stick?
You are enabling the two chemicals inside to react and give off light.
110
What is familiar example of a chemical reaction that gives off both hear and light?
The combustion of propane which is used in bbqs
111
What is an example of a chemical reaction that produces a color change?
A single replacement reaction between silver nitrate and copper. A solid piece of red-brown copper is placed in a clear colorless solution of silver nitrate. The copper replaces the silver and the result is a blue solution of copper nitrate (CuNO3(aq) )with a solid silver precipitate.
112
What is a precipitate?
an insoluble solid
113
When a chemical reaction produces a gaseous substance as one of its products, what does it give off?
It gives off bubbles or fumes that are characteristic of the reaction.
114
What is an example of a chemical reaction that produces a gas?
The reaction between baking soda (NaHCO3(aq) ) and vinegar (acetic acid - CH3COOH(aq) and water)
115
What happens when you mix baking soda and water?
If you mix a baking soda mix (baking soda and water) with vinegar, both substances quickly react and the bubbles that you see are the rapid formation of carbon dioxide gas (C02(g) )
116
True or False, Is Carbon dioxide responsible for the fizz you see in soft drinks?
True
117
What does the burning of paper or wood (a type of combustion reaction) produce?
Carbon dioxide gas as well as water vapour.
118
What does soluble mean?
Able to dissolve.
119
What is precipitate?
the insoluble product that forms a solid that is distinct and separate from a solution.
120
What is an example of a chemical reaction that forms a precipitate?
The double replacement reaction between lead nitrate and potassium iodide. The yellow solid lead iodide quickly clouds up the mixture but will settle to the bottom if left undisturbed for some time.
121
All chemical reactions involve a change in what?
All chemicals reactions involve a change in substances and energy.
122
True or false? Matter and energy are not created or destroyed in a chemical reaction, only transferred.
True
123
What are the four general types of Chemical reactions?
Synthesis, Decomposition, Replacement (also known as Displacement) and Combustion.
124
What is an equation? What does the "=" sign mean?
An equation is a mathematical statement and "=" sign in
| it. Meaning that what is on the left side of the equal sign is equal to what is on the right side of the equal sign.
125
What is a chemical equation?
A chemical equation is a way to represent a chemical reaction. The reactants are given on the left had side and the products are given on the right hand side.
126
What is used instead of an "=" sign in a chemical equation?
instead of an "=" sign, an arrow is drawn between the reactants and the products.
127
What does the arrow mean in an chemical equation?
The arrow means that the reactants get converted into products, sometimes quickly, sometimes slowly. At the end there are no reactants only products.
128
What is the general form of a chemical equation look like?
REACTANTS --------> PRODUCTS
| makes
129
What important information about reactions do Chemical reactions contain?
Name, and relative amounts(or ratios) of reactants and products, and the conditions needed for the reaction to take place.
130
What is a skeletal equation?
The symbolic form of a chemical reaction. It is the shorthand of chemists and lets them easily communicate about chemical reactions with each other around the world.
131
What is a chemical formula?
A way of showing the type(s) and number(s) of elements in a given molecule of a compound.
132
What does a skeletal equation represent?
A skeletal equation represents a reaction using the chemical formulas of the reactants and product.
133
What is a group of two or more atoms held together by chemical bonds?
A molecule
134
What is a pure substance consisting of tow or more different elements?
A Compound
135
What does the general form of a skeletal equation look like?
A + B -------------> C + D
Reactants Products
where A,B,C,D are the chemical formulas of the reactants and products.
136
What are phase tags?
Skeletal equations may also be give PHASE TAGS which show what phase a given chemical is in.
137
What are the different phase tags a given chemical can be in?
Solid(s), Liquid(l), Gas(g) Aqueous(aq)
138
What does Aqueous mean?
Dissolved in water?
139
What are the most common form of chemical equations?
Balanced Chemical Equations are the most common form of chemical equations.
140
How are Balanced chemical equations similar to skeletal equations?
Balanced chemical equations are similar to skeletal equations in that they use chemical formulas and phase tags to describe the reactants and products.
141
How are Balanced equations different from skeletal equations?
Unlike skeletal equations, balanced equations are adjusted so that the law of conservation of mass is upheld.
142
What is the law of conservation of mass?
Mass cannot be created or destroyed.
143
What are numbers placed in front of a chemical formula called?
Coefficients
144
What does the general form of a balanced chemical equation look like?
aA+bB --------->cC+dD
reactants Products Where A,B,C,D are the chemical formulas of the reactants and products and a,b,c,d are their coefficients.
145
What happens in a Synthesis Reaction?
Two or more atoms or molecules combine to form a compound (two or more reactants come together to form a product)
146
What does the general formula for Synthesis Reaction look like?
A + B ----------> AB
| Reactants Product
147
Describe the general formula for Synthesis Reactions
A and B combine to form AB. The physical and chemical properties of A,B and AB are different.
148
Give an example of an Synthesis Reaction?
The formation of water (H2O(1)
2H2(g) + O2(g) ---------------> 2H2O(`1)
Reactants Product
149
How would you balance the reactants and product in the following synthesis
reaction?
N2 + O2 NO + Heat
N2 + O2 2NO
Now the equation is balanced – there are two atoms of nitrogen and two atoms of oxygen on each side of
the equation.
150
Are Decomposition reactions the reverse of synthesis reactions?
Yes
151
Describe Deompostion reactions.
This type of reaction involves a compound that breaks apart into two or more atoms or molecules,
often when heated. The reactant is broken apart to form two or more
products.
152
What is the The general equation for a decomposition reaction?
AB ------> A + B
| Reactant Products
153
Give a specific example of a decomposition reaction.
the breakdown of water into hydrogen and
oxygen gas.
2H2O(l) ------------> 2H2(g) + O2(g)
Reactant Products
154
When does a decomposition reaction happen?
this happens when electricity is passed through the water in a process called electrolysis.
155
What is the clue in the following decomposition reaction that a chemical reaction has occurred?
2H2O(l) ------------> 2H2(g) + O2(g)
It produces a gas
156
How would you balance the reactant and products in the following
decomposition reaction of hydrogen peroxide (H2O2) into water and oxygen gas?
H2O2 ----------------> H2O + O2
First make the inventory of atoms.
Since the oxygen is in reactants is in two different molecules this time, we do not have to change both.
We can simply change the H2O. If we double the H2O, we get H2O2 ---------> 2H2O + O2
In order to balance the left side, we now simply need to double the H2O2
2H2O2-------------------> 2H2O + O2
157
What are the 2 types of replacement reactions ?
single replacement reactions and
| double replacement reactions
158
What are single replacement reactions?
a single uncombined element C replaces another element in a compound AB.
159
What is the general equation for a single replacement reaction?
C + AB ---------> CB + A
| Reactants Products
160
What happens in a single replacement reaction if C is a metal? What happens is C is a non-metal?
C is a metal, then it replaces the metal part of AB (which is always A) and that if C is a
non-metal, then it replaces B (which is always a non-metal).
161
Give a specific example of a single replacement reaction?
CuO(s) + H2(g) ----------------> Cu(s) + H2O(l)
Reactants Products
Copper oxide is black and solid copper is reddish-brown
IMPORTANT FACT: This reaction involves a change in colour which is a clue that a chemical
reaction has occurred.
162
How would you balance the reactants and products in the following single replacement reaction of
aqueous potassium iodide (KI) and aqueous fluorine (F2) into aqueous iodine (I2) and aqueous potassium
fluoride (KF)?
KI (aq) + F2(aq) --------------> I2 (aq) + KF(aq)
First make the inventory of atoms.
Since you need two I atoms, you can double the KI on the left side to get: 2KI(aq) + F2(aq) -------> I2(aq) + KF(aq)
double the KF on the right side to get:
2KI(aq) + F2(aq)--------> I2(aq) + 2KF(aq)
163
What is a double replacement reaction (also called a metathesis reaction)?
It involves two compounds that form two new compounds through the exchange of their anions and
cations. As in single replacement reactions, only cations can replace cations and only anions can replace anions.
164
What is the general formula for a double replacement reaction?
AB + CD ------------> AD + CB
Reactants Products
A and C are cations and B and D are anions. Therefore only A can replace C and only B can replace D.
Typically this type of reaction results in the formation of a
precipitate.
165
What is a specific example of a double replacement reaction?
A specific example of a double replacement reaction is the reaction between solutions
of calcium oxide II (CaO) (also known as quicklime) and hydrochloric acid:
CaO(s) + 2HCl(aq)------------------> CaCl2(s) + H2O(l) + heat
Reactants Products
166
Explain the double replacement reaction between the solutions of calcium oxide II (CaO) (also known as quicklime) and hydrochloric acid.
When solid calcium (II) oxide is treated with a colorless solution of hydrochloric acid,
calcium chloride and water are produced. The water can be evaporated to recover the solid compound, calcium chloride
IMPORTANT FACT: This reaction produces heat which is a clue that a chemical reaction has
occurred.
167
What is an acid–base reaction?
a special type of double replacement reaction that occurs between an acid and a base.
168
Describe acids.
Acids can generally be regarded as having a sour taste,
| such as vinegar and lemon juice, and can react with many (but not all) metals
169
Describe bases.
s have a bitter taste, such as baking soda and feel slippery like soap
170
What is interesting about the acid and bases react to each other?
When the react together, each is capable to cancel out (or neutralize) the acidic or basic properties of the other
Acid and bases react to each other in many ways including neutralization reactions.
171
What is an example of an acid based reaction?
The reaction of hydrochloric acid (HCI) with sodium hydroxide (NaOH)
HCI (aq) + National OH (aq) ---------> H2O (I) + NaCI (aq)
Important fact- by removing the water from NaCI (aq) you could have NaCI (s) - table salt
172
What is pH?
pH is a measure of the acidity of a solution in terms of concentration of hydrogen ions (protons) H+ and is commonly expressed using the pH scale.
173
What is the pH scale?
pH scale ranges from 0-14 and describes how acid or basic something is.
174
What does a pH of 7 mean?
A neutral substance (neither acid nor basic) such as pure water.
175
What does a pH of less than 7 mean?
Means the solution is acidic.
176
What does a pH of more than 7 mean?
Means the solution is basic.
177
True or false? The higher the pH the more basic the solution is.
True
178
When does a combustion reaction occur?
When oxygen (O2) combines with another compound (called fuel) to for water and carbon dioxide as the most common products.
179
What are some other products of a combustion reaction?
Carbon monoxide, soot (in burned carbon), sulfur dioxide, nitrogen oxides.
180
What is the source of oxygen for most combustion reactions?
Air
181
Whathe happens to a candle without oxygen?
It goes out.
182
What is candle wax (paraddin) composed of?
Chains of connected carbon atoms surrounded by hydrogen atoms.
183
What happens when you light a cndle?
The heat of the flame turns solid we into wax vapour (gas form). The vaporized wax molecules are able to react with the oxygen in the air.
184
What are the major products from a burning candle?
Carbon dioxide and water vapour, soot (which creates the yellow flame), and some carbon monoxide.
185
What is an example of incomplete combustion?
A candle flame.
186
What is an examale of a complete combustion?
| Show as a chemical equation
Burning of butane
C4 +H10----> CO2+H2O
Butane/oxygen-carbon dioxide/water
IMPORTANT FACT - this reaction involves a change in temperature which is a clue a chemical reaction has occured.
187
What is important to know about combustion reactions?
That they are esoteric meaning they produce heat.
188
When do people use combustion reactions? Give examples
For heat and light. Burning wood natural gas welders torch.
189
What are petrochemicals?
Compounds that are created using carbon based sources such as crude oil, natural gas, coal or renewables.
190
where can you find polyethylene?
Most common ingredient in plastic. Bottles, packaging and consumer goods.
191
Where is Down Canada manufacturing located?
Alberta
192
How do you make polyethylene?
Take natural gas liquids and store in underground caverns. Use fractionation to separate the NGL into components: ethane, propane, butane, hydrocarbons. The ethane heat up and cracked into ethylene in a thermal cracker. Finally ethylene is turned into polyethylene.
