Elements and compounds in our surroundings

Chemistry I Stage II
Ms. Claudia Barahona
Elements & compounds in our surroundings

Stage I1 Chemical reactions in our surroundings
Formative Objective: The student identifies the chemical name and formula of elements and compounds present in our daily lives, to reflect on the effects and importance of these substances in our bodies and surroundings.
Elaborated by: QFB. Claudia Barahona

TOPICS
Classification of elements in : metals, nonmetals and metalloids
Classification of compounds by the number of elements and chemical function.
Elements present in the human body and acquisition sources.
The effects and uses of chemical compounds in our daily lives

COMPETENCES
Generic Competences:
4. Listens, interprets, and emits pertinent messages in different situations using mediums, codes and appropriate tools.
 Express ideas and concepts through
 Identifies the main ideas in a text or an oral speech, and deduce conclusions from them.
5. Develops innovations and proposes solutions from established methods.
 Follows directions and procedures objective.
 Synthesizes evidences obtained with experimentation to produce
 Uses the information and communication technologies to
Disciplinary Competences:
2. The student bases opinions about the impact of science and technology in his daily life assuming ethical considerations.
10. The Student relates the symbolic expressions of a phenomenon of the sight or using scientific instruments or models.

Activity 2.1 Exploring your knowledge

What is an ELEMENT?
oA pure substance composed of only one type of atom.
oCannot be broken down into another substance by chemical or physical means.

Compounds
A pure substance consisting of 2 or more elements chemically combined, in a definite composition that can be broken down into a simpler substance, using chemical methods of separation.
Chemical methods:
◦Electrolysis
◦REDOX reactions
◦Catalysis

Dmitri Mendeleev (1869)
http://www.chem.msu.su/eng/misc/mendeleev/welcome.html
The periodic table
Arrangement of elements by increasing
atomic number

http://www.chem.msu.su/eng/misc/mendeleev/welcome.html
K
Au
P
Sn
Cu
Ni
Pb
N
Act 2.1 Q 4

Representative elements
Transition
Metals

Chemical Symbols
Are one or two-letter abbreviations for the names of an element.
ONLY THE FIRST LETTER IS CAPITALIZED.
If the symbol has a second letter, it is lowercase SO THAT WE KNOW WHEN A DIFFERENT ELEMENT IS INDICATED.
CO Co
CARBON MONOXIDE
Cobalt
The symbol of Carbon is C, the symbol of sulfur S. However the symbol of Cesium is Cs not CS. Why not?

Origin of some of the elements name
Most of the chemical symbols use letters from the current name, some are derived from their ancient name.
Other elements are named after planets, mythological figures, colors, minerals, geographical location and famous people.
Act 2.1
Part II

Activity 2.2 Acquisition of knowledge
Vocabulary terms

Vocabulary terms
1.Periodic table
2.Period
3.Group or family
4.Chemical symbols
5.Representative elements
6.Transition elements
7.Metals
8.Nonmetals
9.Metalloids
10.Malleable
11.Ductile
12.Element
13.Compound
14.Binary compound
15.Ternary compound
16.Polyatomic compound
17.Acids
18.Bases
19.Oxides
20.Salts
21.Valence electrons
22.Ionic bond
23.Covalent bond

Typical amounts of essential elements in:
Human body

Typical amounts of essential elements in:
Planet
Universe

Act 2.2 Part III
Element
Real case intoxication (lethal dose)
Source of acquisition
Symptoms
First aid in case of intoxication
Arsenic (As)
Can be administered through oral via such as food, drinks, etc.
In adults is estimated to be 70 to 200 mg or 1 mg/kg/day.
Headaches, confusion, severe diarrhea, drowsiness. Convulsions.
vomiting, blood in the urine, cramping muscles, hair loss, stomach pain, and more convulsions. The final result of arsenic poisoning is coma and death.
Dimercaproland dimercaptosuccinic acid are chelating agents that sequester the arsenic away from blood proteins.

Act 2.2 Part III
Element
Symptoms
Chromium (Cr)
Drinking water,
Ranges between 1900 and 3300 μg/kg.
Chromate dye company. Cr often used to manufacture, amongst other things, leather products, paints, cement, mortar and anti- corrosives.
Can lead to DNA damage. After it reaches the blood stream, it damages kidneys, liver and blood cells, Hemolysis, renal and liver failure are the results of these damages.
Appropriate supportive measures may include ventilatory support, cardiovascular support, and renal and hepatic function monitoring.
Check the 7 diatomic molecules

Act 2.2 Part III
Element
Symptoms
Mercury
Consumption of fish is by far the most significant source of ingestion-related mercury exposure in humans and animals, although plants and livestock also contain mercury due to bioconcentration of mercury from seawater, freshwater, marine and lacustrine sediments, soils.
Sensory impairment (vision, hearing, speech), disturbed sensation and a lack of coordination. Damage to the brain, kidneys and lungs
Immediate chelation therapy,
Check the 7 diatomic molecules

The Periodic Table
 A map of the building block of matter.
1
IA
18
VIIIA
1
1
H
1.00797
2
IIA Periodic Table 13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA
2
He
4.0026
2
3
Li
6.939
4
Be
9.0122
5
B
10.811
6
C
12.0112
7
N
14.0067
8
O
15.9994
9
F
18.9984
10
Ne
20.179
3
11
Na
22.9898
12
Mg
24.305
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8 9
VIIIB
10 11
IB
12
IIB
13
Al
26.9815
14
Si
28.086
15
P
30.9738
16
S
32.064
17
Cl
35.453
18
Ar
39.948
4
19
K
39.102
20
Ca
40.08
21
Sc
44.956
22
Ti
47.90
23
V
50.942
24
Cr
51.996
25
Mn
54.9380
26
Fe
55.847
27
Co
58.9332
28
Ni
58.71
29
Cu
63.54
30
Zn
65.37
31
Ga
65.37
32
Ge
72.59
33
As
74.9216
34
Se
78.96
35
Br
79.909
36
Kr
83.80
5
37
Rb
85.47
38
Sr
87.62
39
Y
88.905
40
Zr
91.22
41
Nb
92.906
42
Mo
95.94
43
Tc
[99]
44
Ru
101.07
45
Rh
102.905
46
Pd
106.4
47
Ag
107.870
48
Cd
112.40
49
In
114.82
50
Sn
118.69
51
Sb
121.75
52
Te
127.60
53
I
126.904
54
Xe
131.30
6
55
Cs
132.905
56
Ba
137.34
57
La
138.91
72
Hf
178.49
73
Ta
180.948
74
W
183.85
75
Re
186.2
76
Os
190.2
77
Ir
192.2
78
Pt
195.09
79
Au
196.967
80
Hg
200.59
81
Tl
204.37
82
Pb
207.19
83
Bi
208.980
84
Po
[210]
85
At
[210]
86
Rn
[222]
7
87
Fr
[223]
88
Ra
[226]
89
Ac
[227]
104
Ku
[260]
105 106 107 108 109
http://www.chemsoc.org/viselements/pages/periodic_table.html

Reading the Periodic Table: Classification
Nonmetals, Metals, Metalloids, Noble gases

Across the Periodic Table
 Periods: Are arranged horizontally across the
periodic table (rows 1-7)
 These elements have the same number of valence shells.
1
IA
18
VIIIA
1
2
IIA
13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA
2
3
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8 9
VIIIB
10 11
IB
12
IIB
4
5
6
7
2nd Period
6th Period

Down the Periodic Table
Family: Are arranged vertically down the periodic table (columns or
group, 1- 18 or 1-8 A,B)
These elements have the same number electrons in the outer most shells, the valence shell.
1
IA
18
VIIIA
1
2
IIA
13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA
2
3
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8 9
VIIIB
10 11
IB
12
IIB
4
5
6
7
Alkali Family:
1 e- in the valence shell
Halogen Family:
7 e- in the valence shell

Infamous Families of the Periodic Table
 Notable families of the Periodic Table and some important members:
1
IA
18
VIIIA
1
2
IIA
13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA
2
3
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8 9
VIIIB
10 11
IB
12
IIB
4
5
6
7
Alkali
Alkaline
(earth)
Transition Metals
Noble Gas
Halogen
Chalcogens

Metals appear to the left of the dark ziz-zag line on the periodic table. Most metals are solid at room temperature.
Properties of metals

Metals have luster. This means they are shiny

Ductile
metals can be drawn into wire.
COPPER

Malleable
metals can be hammered into sheets
ALUMINUM

Metals have a high melting point. They are also very dense.

Conductors
Metals are good conductors of electricity and heat

A chemical property of metal is its reaction with water and oxygen. This results in corrosion and rust.

•Shiny
•Solids at room T° (except Hg)
•Luster
•Good conductors of heat and electricity
•Malleable (sheet)
•Ductile (wires)
•High melting points
•High density

Nonmetals occur to the right of the dark zig-zag on the periodic table. Although Hydrogen is in family 1, it is also a nonmetal. Many nonmetals are gases at room temperature.
Properties of Non metals

Nonmetals do not have luster; they are dull.
Properties of Non-metals

Brittle
Nonmetals are brittle so they break easily. This means nonmetals ARE NOT ductile or malleable.

Nonmetals have low density.

They also have a low melting point. This is why they are poor conductors of heat and electricity.

Properties of nonmetals
Nonmetals:
Lacks of luster
Low melting point
Low density
Bad conductors of heat or electricity

Metalloids can be found clustered around the dark zig-zag line that separates metals and nonmetals.
Properties of Metalloids

Metalloids (metal- like) have properties of both metals and nonmetals.

Metalloids are solids that can be shiny or dull.

They conduct electricity and heat better than nonmetals but not as well as metals.

Metalloids are malleable and ductile

Properties of metals, nonmetals and metalloids
Metalloids:
Possess characteristics of both metals and nonmetals
Semiconductors

What is a COMPOUND?
oA substance in which two or more different elements are CHEMICALLY bonded together.

Types of Compounds
•A compound with 2 different elements
•NaCl – Sodium Chloride
Binary
•A compound with 3 different elements
•HClO Hypochlorous Acid
Ternary
•A compound with 3 or more elements
•NaHCO3 Sodium Bicarbonate
Polyatomic

Classification of Inorganic Compounds
INORGANIC COMPOUND
CLASSIFICATION
ELEMENTS
Metal
Non-metals
Metalloids
COMPOUND
Salt
Oxide
Base
Acid
Others*

ACIDS
Contain the H+ ion and a non-metal ion or polyatomic ion in an aqueous (aq) solution
CATION
ANION
HCl -> Hydrochloric acid
H2SO4 -> Sulfuric acid
Some characteristics
Taste
Sour
Feel
May Sting
Litmus
Red
Phenolphthalein
Colorless
Neutralization
Neutralizes bases

Strong acids
6 common strong acids:
•Perchloric acid
HClO4
•Sulfuric acid
H2SO4
•Hydroiodic acid
HI
•Hydrobromic acid
HBr
•Hydrochloric acid
HCl
•Nitric acid
HNO3

BASES
Contain a metal ion and the (OH)- ion in an aqueous (aq) solution
CATION
ANION
Characteristics of bases
Taste
Bitter, chalky
Feel
Soapy, slippery
Litmus
Blue
Phenolphthalein
Pink
Neutralization
Neutralizes acids
No special naming rules for bases.
Ex. KOH -> potassium hydroxide
Ex. NH4OH -> ammonium hydroxide

OXIDES
Binary compounds that contain a metal or non metal ion and the O-2 ion, normally in a solid state (s)
Al2O3 is aluminum oxide ( Ionic M-NM)
CO carbon monoxide (Covalent NM-NM)

SALTS
Contain a metal ion (Not H+) and non-metal ion or polyatomic ion (NOT (OH)- nor, O-2 )
1. normally in a solid state, (s), or in an aqueous, (aq), solution
2. SALTS ARE FORMED AFTER THE NEUTRALIZATION OF AN ACID BY A BASE
Example:
LiF lithium fluoride
MgCr2O7 magnesium dichromate
Pb(ClO3)4 lead (IV) chlorite
CATION
ANION

Others
Ionic compounds
Covalent compounds

Ionic compounds
Ions are held together by strong electrical attractions between the opposite charges called ionic bonds.
◦Cation= Metal
◦Anion= Nonmetal
The sum of the ionic charges
on the formula is always
zero!!
CATION
ANION

Covalent compounds
Forms when atoms of 2 nonmetals share electrons.
Held together by the sharing of electrons called covalent bond.
When 2 or ore atoms share electrons they form a molecule.
CATION
ANION

Review
Classify the following compounds based on the number of elements and function.
1.AgOH
2.MgO
3.KOH
4.CaF2
5.Na2CO3
6.Na3PO4
7.CaCO3
8.H2SO4
9.ClO3
10.SO3
11.Fe203
12.Mg(OH)2
13.HNO3
14.PbO2
15.CO2
16.Na2O
17.HBr

Elements in their natural state
Simplest kind of pure substance that contains only one type of matter and cannot be broken down by chemical methods.
Most of the elements in their natural state are found as compounds.
Diatomic molecules
7 elements are found as diatomic molecules:
◦H2, N2, O2, F2, Cl2, Br2 e I2

Chemical compounds by number of elements

Compounds
Two or more elements chemically combined.

Number of elements
Compounds can be classified according to the number of different elements chemically combined as:
◦Binary (two elements)
Ex: NaCl, FeS, H2O.
◦Ternary (Three elements)
Ex: NaOH, HClO4, H2SO4
◦Polyatomic (four or more)
Ex: NaHCO3, (NH4)2SO4, NaHSO3

Classification of compounds by their function
compounds
Acids
Bases
Oxides
Salts

Acids and bases
Lemons
Grapefruits
Vinegar
Sodium hydroxide
Antiacids Acetic acid

Acids
Arrhenius theory: Substance that dissolves in water and produces hydrogen ions (H+).
Bronsted-Lowry: Proton donor substances.

Properties of Acids
Sour taste.
Turns litmus paper indicator red.
Turns phenolphtalein indicator colorless.
Corrode some metals.

Bases
Arrhenius theory: Substance that dissolves in water and produces hydroxide ions (OH-).
Bronsted-Lowry: Proton acceptor substances.

Properties of Bases
Bitter taste.
Slippery feel (soaps).
Turns litmus indicator blue.
Turns phenolfphtalein indicator pink.

Oxides
Chemical binary compounds with one or more oxygen atoms combined with another element.

Salts
Ionic compound that contains a metal ion or NH4+ and a nonmetal or polyatomic ion other than OH-.

Chemical compounds by type of bond

Ionic compounds
Consists of positive ion (metal) and negative ion (nonmetal).
Metal - Nonmetal

Covalent compounds
Nonmetal – Nonmetal
When 2 or more atoms share electrons they form a molecule.

Electronegativity
Relative ability of an atom to attract the share electrons by itself.
In a period, it increases.
In a group it decreases.
Nonmetals, Fluorine 4.0 and oxygen 3.5 have the highest electronegativites.
Metals Cesium and Francium have the lowest electronegativities.

Electronegativity
Increasing electronegativity
Increasing electronegativity
Representative elements
Transition Metals

Polarity
•Describes how electrons are shared between atoms .
•Electrons are not always shared equally between two bonding atoms.
•One atom might exert more of a force on the electron than the other, electronegativity.
•The unequal sharing of electrons within a bond leads to the formation of polarity.

Polarity of bonds
Nonpolar covalent bond: Bond between atoms with identical or very similar electronegativities.

Polarity of bonds
Polar covalent bond: Electrons are shared unequally.

Summary of bonds

Topic: Chemical elements and compounds in your body and surroundings
Compound
Formula
Elements involved
Classification by # of E
Classification by chemical function
Carbon dioxide
CO2
Carbon
Oxygen
Binary
Oxide
Hydrochloric acid
HCl
Hydrogen
Chlorine
Binary
Acid
Vinegar (Acetic acid)
CH3(COOH)
Carbon
Hydrogen
Oxygen
Ternary
Acid
Table salt (sodium chloride)
NaCl
Sodium
Chlorine
Binary
Salt

Topic: Chemical elements and compounds in your body and surroundings
Compound
Formula
Elements involved
Classification by # of E
Classification by chemical function
Sodium bicarbonate
NaHCO3
Sodium
Hydrogen
Carbon
Oxygen
Polyatomic
Salt
Sodium hydroxide
NaOH
Sodium
Oxygen
Hydrogen
Ternary
Base
Calcium oxide
CaO
Calcium
Oxygen
Binary
Oxide
Nitrogen monoxide
NO
Nitrogen
Oxygen
Binary
Oxide

1. An ionic compound is a chemical compound in which ions are held together by the electrostatic force between oppositely charged ions.
2. An ionic compound is form by a positively charge ion called a cation, which is always a metal and a negatively charged ion called a anion which is always a nonmetal or a polyatomic ion when we have 2 or more nonmetals together with a charge.

3. The main difference between ionic and covalent compounds is that ionic compounds is composed of a metal bonded to a nonmetal while a covalent compound is a nonmetal bonded to a nonmetal.
4. In ionic compounds there is a complete transference of electrons.
5. In covalent compounds electrons are being shared.

Compound
Classification
Compound
Classification
BaCl2
Ionic
Cl2O
covalent
N2O4
Covalent
KF
Ionic

Compounds according to the type of bond

Ionic compounds
Consists of positive ion (metal) and negative ion (nonmetal).

Covalent compounds
When 2 or more atoms share electrons they form a molecule.

Metallic bonds
Bonding of atoms in solid metallic crystals.
A three-dimensional array of positive ions that remain fixed in the crystal lattice while loosely held valence electrons move freely throughuot the crystal.
Sharing a “sea of ve-”.
e- are free to move.

Properties
Good conductors of electricity and heat
Insoluble in water
Malleable (sheets)
Ductile (wires)
Shiny

Elements and compounds in our surroundings

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