Chemistry Flashcards
1
Q
Test tube brushes?
A
Used to clean test tubes and other equipment
2
Q
Bunsen Burner
A
Heat or ignite materials
3
Q
Wire Gauze
A
Supports equipment on a ring clamp
4
Q
Ring stand
A
Supports equipment
- Attach clamps to it to hold beakers
5
Q
Florence Flask
A
Container for liquids
- May be heated
6
Q
Utility Clamp
A
Fastens to retort stand
- holds test tubes
7
Q
Spatulas
A
- To transfer solids
8
Q
Wash bottle
A
- Squeeze to dispense distilled water
9
Q
Clay Triangle
A
Supports crucible on a ring clamp
9
Q
Test Tube
A
Holds small amounts of liquids and solids
- May be heated
10
Q
Grad Cylinder
A
Measuring liquids accurately
11
Q
Iron Ring
A
Fastens to retort stand
- Holds equipment
12
Q
Mortar and Restle
A
Grinds solids into powder
13
Q
Test Tube Rack
A
Holds test tubes upright
14
Q
Test Tube Holder
A
To hold and transfer test tubes
15
Q
Evaporating dish
A
Container to evaporate small amount of liquid
16
Q
Watch glass
A
Cover for beaker
- Can hold small amounts of liquids
17
Q
Glass Plate
A
Covers for beakers and glass bottles
18
Q
Funnel
A
aids in pouring liquids
- support for filter paper while filtering
19
Q
Stir Rod
A
to stir chemicals together
20
Q
Beaker Tongs
A
to hold and pick up beaker
21
Q
Crucible Tongs
A
to pick up and hold a crucible and lid
22
Q
Erlenmeyer Flask
A
holds liquids
-useful to swirl/mix chemicals
- may be heated
23
Q
Forceps
A
to pick up small solids
24
Beaker
to hold liquids or solids
- may be heated
25
Pipette
To accurately measure and transfer iquids
26
Dropper
To transfer small amount of liquids
27
Crucible
To hold small solids while heating to high temperatures
28
Rules in Lab
Never perform an experiment
without the instructions or
approval of
your teacher.
Before starting an
experiment,
read all of the
directions.
29
Rules in Lab
wear goggles
30
9 lab rules
1. Liquid waste must be disposed of in proper containers
2. Broken Glass in broken glass container
3. Report all accidents
4. Never small or taste any ingredients
5. Never put out chem fire with water use extinguisher
6. Never leave your lab area unattended
7. Clean spills with WET SPONGE NOT PAPER TOWEL
8. Never return excess chemicals
Keep clean equipment
31
WHMIS
The Workplace Hazardous Materials
Information System (WHMIS) are laws created
in 1988 to inform employers and workers about
hazardous products or chemicals they may be
exposed to at work and reduce workplace
injuries and illnesses.
32
Compressed Gas (rolling pin)
Risks - Can explode
Precautions - Handle with care don't drop or puncture
33
Poisonous and Infectious (skull and bones)
Risks - Can cause death or acute toxicity if exposed to small amt of hazard
Precautions - Cover skin and handle with caution
34
Corrosive Material (Hand and pipe)
Risks - Can destroy skin
Precautions - Wear propor ppe
35
Dangerously Reactive Material (R)
Risks - Explosions, fire, extreme heating
Precautions- Keep way from sparks, heat and direct sunlight
36
Oxidizing Material (line,under circle with flame)
Risks - Can feed fire, making it much hotter
Precautions -Keep away from combustible materials like wood and flammable materials
37
Biohazardous (circle and semi circles)
Risks - Harmful to our health, can give serious illness
Precautions: wash hands often
38
Flammable and Combustible Material (line and flame)
Risks - Can burst into flames
Precautions -Handle with care, keep way from heat
39
Poisonous and infectious (T)
Risks - eyes, skin and lung irritation and cancer
Precautions - avoid contact with skin or eyes
40
Matter
Matter is anything that has mass and takes up
space
41
Mass
Mass is a measure of the quantity of matter in an
object
42
Volume
Volume is a measure of how much space an object
takes up
43
Particle Arrangement in solids
In solids, the particles are
close together (stronger
attractive force)
44
Particle Arrangement in liquids
In liquids, the particles are
farther apart (weaker
attractive forces)
45
Particle Arrangement in gases
In gases, particles are very far
apart (very weak forces)
46
The Particle Theory
The Particle Theory is a way to describe the
structure of matter and its behavior.
47
Particle Theory (4)
All matter is composed of very tiny objects called
particles
All particles have space between them
Particles present in matter are always in motion
The particles in a substance attract each other
48
Particles in ice
In ice, the particles
vibrate but cannot move
around. The particles are
very attracted to each
other.
49
Particles when heat is added
When heat is added, the
particles slide past each
other forming liquids
and break away from
each other forming
gases as more heat is
added.
50
Matter
Matter has mass and takes up space
51
Whats matter made of
Particles
52
What is a property
A property is a characteristic that describes a
substance.
53
How can substances be classified
Substances can be classified as pure substances or
mixtures, depending on how their particles are
arranged.
54
Matter is two categories
Mixtures and Pure substances
54
Pure substances are
Compounds and elements
55
Mixtures are
heterogeneous mixtures and homogeneous mixtures (uniform)
56
heterogeneous mixtures
Mechanical mixtures and suspensions
57
homogeneous mixtures (uniform)
solutions
57
Compounds?
a thing that is composed of two or more separate elements; H2O and CO2
57
elements?
A substance that cannot be broken down into simpler substances by chemical means; Hydrogen, Carbon and Oxygen
58
heterogeneous mixtures?
A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture; choc chip cookies, salad and pizza
59
homogeneous mixtures (uniform)
A homogeneous mixture is a gaseous, liquid or solid mixture that has the same proportions of its components throughout a given sample. It is uniform in composition throughout; Blood, Air and Sea water
60
Mechanical Mixtures
When different kinds of matter are visible in the mixture it is called a mechanical mixture (or heterogeneous mixture). In a mechanical mixture, the particles are unevenly distributed in groups. Examples of mechanical mixtures include a toy box, cereal and milk or a pizza.
61
Suspensions
A suspension is a heterogeneous mixture of two or more substances. Here, the particles are suspended throughout the solution in bulk and can be easily seen by naked eyes. In it, particles of the solute do not dissolve in the solution and are rather suspended; Mud, sand in water and chalk in water
62
Mixtures
Have two or more different types of particles
Three kinds of mixtures: mechanical mixtures,
solutions and suspensions.
63
Solutions
In a solution the different substances that make it up
are not individually visible; sugar dissolved in tea or coffee
When you stir the sugar into the tea it appears to disappear
64
A physical Property
A physical property describes a
characteristic of a substance that can be
observed or measured.
65
Physical Properties?
Colour, Taste, Odour, Clarity, Lustre, Texture, Form, Brittleness, Hardness, Malleability, Ductility, Viscosity, Conductivity, Cohesion and Adhesion and Density
66
Chemical Property?
A chemical property describes the ability of a substance to
change into a new substance or substances; Chemical properties include how a substance interacts with
other substances, heat or light.
67
Chemical Change?
A chemical change always results in the formation of a new
substance or substances.
68
Chem reaction?
A chemical reaction is a process in which a chemical change
occurs.
69
Chemical properties can be observed only when a chemical
change has occurred.
Statement
70
Slope Formula?
(y2 -y1)/(x2 - x1) = rise/run = vert change/ horizontal change
71
Chopping a piece of wood
Physical Change
72
Burning a piece of wood
Chemical
73
What's an atom
An atom is the smallest part of
an element that has all the
element’s properties.
74
Atomic Theory
Atomic theory is the study of nature of atoms and how they
combine to form all types of matter.
75
Democritus
Democritus hypothesized that breaking down rock into
powder would reduce it to tiny bits of matter that could not be
broken down more.
76
DALTON (1766-1844)
Dalton proposed that
atoms were like small
spheres.
77
DALTON’S ATOMIC THEORY
All matter is made up of small, indivisible particles called
atoms
All the atoms of an element are identical in properties such as
size and mass.
Atoms of different elements have different properties.
Atoms of new different elements can combine in specific ways
to form new substances.
78
J.J THOMSON (1856-1940)
Thompson researched that atoms
may be made from a combination
of particles
Experimented with cathode ray
tubes, heated a metal in the tube
and produced negatively charged
particles
These particles were later called
electrons.
79
THOMPSON’S MODEL OF THE ATOM
Thompson proposed atoms of
all elements contained
electrons.
80
ERNEST RUTHERFORD (1891-1937)
Conducted a famous experiment called
the gold foil experiment to test
Thompson’s model.Rutherford’s experiment proved that
atoms have a nucleus in the center of
the atom.
The nucleus has a positive charge.
81
JAMES CHADWICK (1891-1974)
Chadwick discovered that nucleus contains neutral (0)
particles as well as positively (+) charged particles.
82
NIELS BOHR (1885-1962)
Bohr transformed
Rutherford’s model into one
of the models that are used
today.
This model is known today
as a Bohr atom or a Bohr
diagram model.
Electrons are arranged in
energy levels or shells,
orbits.
83
BOHR ATOM
Bohr discovered that electrons jump between electron shells
by gaining or losing energy.
Each shell can contain a specific number of electrons.
The first shell holds 2 electrons, the second and third shell
contains 8, and the fourth shell contains 8. e.g.
nucleus)2e-)8e-)8e-)8e-
84
THE QUANTUM MECHANIC MODEL
This model is the most
advanced and accurate
model of the atom.
In this model, electrons do
not exist as tiny points in the
atom. Electrons exist in
specific energy levels, but
they surround the positively
charged nucleus.
85
Compounds
A compound is a substance made up of two or
more elements that are chemically combined.
86
Two Types of Compounds
Ionic
Molecular
87
Ionic Compounds
Ionic compounds are pure substances usually
consisting of at least one metal and one
non-metal.
88
Properties of Ionic Compounds
Have high melting points
Form crystals
Dissolve in water to form solutions that
conduct electricity.
All ionic compounds are solids at room
temperature.
89
Forming Ionic Compounds
While combining, each atom changes into an
ion. Ions form when one or more electrons
move from a metal to a non-metal.
90
Ionic
The sodium atom loses an electron to become a
positive ion (cation), and the chlorine gains an
electron to become a negative ion (anion)
91
Why do ions form?
Atoms gain or lose electrons to form a stable octet
This refers to the outer electron shell being filled to its capacity
Atoms with full outer electron shells are stable
(i.e. ALL Noble Gases are stable elements)
Atoms will move the fewest possible electrons to obtain a
complete outer shell
The electrons in the outer shell are called valence electrons
92
Molecular Compounds
When non-metals combine, a pure substance called a
molecular compound is formed.
In molecular compounds, the atoms share electrons to
form small groups called molecules.
Examples of molecular compounds include water, carbon
dioxide, and table sugar
93
Chemical Families?
Alkali metals.
Alkaline earth metals.
Halogens.
Noble gases
94
Alkali metals.
Li, Na, K
1 valence
Metal
Reactive metals
95
Alkaline earth metals
Mg, Ca, Be
2 valence
Metal
Reactive Metal
96
Halogens
F, Cl, Br
7 valence
non-metals
reactive gases
97
Nobel gases
Ne, He, Ar
8 valence (except He has 2)
non metals
non reactive gases
