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KIMIA DASAR 1
(FPU 617107)
BAGIAN 1
Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
SUMBER BELAJAR 2
th
Raymond Chang 2010. Chemistry 10 Edition. McGraw
Hill Higher Education, New York.
Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
ILMU KIMIA 3
APAKAH ILMU KIMIA ?
Ilmu yang mempelajari materi dan perubahan-
perubahan yang terjadi padanya
A B C
D E F
Jurusan TJurusan Teknologi Hasil Pertanian eknologi Hasil Pertanian
Fakultas Pertanian Universitas LampungFakultas Pertanian Universitas Lampung
4
SEJARAH PERKEMBANGAN (ILMU) KIMIA:
1. Kesehatan dan Kedokteran,
Sanitasi, Obat bius, antibiotic dan vaksin; terapi gen,
dan obat-obatan tanpa efek samping
2. Energi dan Lingkungan
Minyak bumi, Greenhouse gas; Renewable and green
energy
3. Material dan Teknologi
Polimer, keramik, liquid kristal, Coating; Komputer,
silikon chip.
4. Pangan dan Pertanian
Pupuk, pestisida, herbisida; Rekasaya genetik (GMF);
Pengolahan hasil-hasil pertanian.
Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
BAGAIMANA MEMPELAJARI (ILMU) KIMIA: 5
1. Baca materi kuliah terlebih dahulu sebelum masuk
kelas.
2. Datang kuliah teratur dan catat bahan yang
diajarkan dengan baik.
3. Ulang topic yang anda peroleh dikelas pada hari
yang sama.
4. Berpikir secara kritis, apakah anda benar-benar
sudah mengerti dengan suatu istilah atau suatu
persamaan.
5. Jangan ragu untuk bertanya pada dosen atau asisten
doses untuk mendapatkan bantuan
Jurusan TJurusan Teknologi Hasil Pertanian eknologi Hasil Pertanian
Fakultas Pertanian Universitas LampungFakultas Pertanian Universitas Lampung
KLASIFIKASI MATERI 6
MATERI (MATTER):
• Segala sesuatu yang menempati ruang dan mempunyai
berat
ZAT (SUBSTANCE):
• Salah satu bentuk dari materi yang mempunyai
komposisi tertentu (tetap) dan sifat tertentu
(berbeda) - emas, gula, air, oksigen
CAMPURAN (MIXTURE):
• Kombinasi (gabungan) dua zat atau lebih, dimana zat-
zat tersebut mempertahankan identitas masing-masing
1) Campuran Homogen:
• Susunan keseluruhan seragam - gula dalam air
2) Campuran Heterogen:
• Susunan tidak seragam - tepung dalam air
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Fakultas Pertanian Universitas Lampung
ZAT (SUBSTANCE): 7
1) Unsur (Element) - Atom
• Suatu zat yang tidak dapat dipisahkan lagi
menjadi zat-zat yang lebih kecil secara kimia.
• 117 unsur telah diketahui (Daftar Periodik), 83
alami, sisanya buatan manusia
• Penamaan dengan 2 huruf/abjad, dimana huruf
pertama selalu huruf besar.
2) Senyawa (Compound) - Molekul
• Gabungan dari beberapa unsur yang terikat secara
kimia dengan perbandingan tetap
• Dapat dipisahkan menjadi unsur-unsurnya (murni)
secara kimia Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
8
Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
STRUKTUR ATOM DAN MOLEKUL 9
TEORI ATOM DALTON
1) Setiap unsur (element) tersusun partikel terkecil
disebut atom.
2) Setiap atom pada tiap unsur adalah identik (ukuran,
berat, dan sifat).
3) Senyawa (compound) tersusun dari atom lebih dari
satu unsur dengan jumlah kombinasi yang sederhana
dan utuh.
4) Reaksi kimia hanya meliputi pemisahan,
penggabungan, dan pengaturan atom, tidak untuk
menciptakan atau menghancurkan atom (hukum
kekekalan atom/massa)
Jurusan Teknologi Hasil Pertanian
Fakultas Pertanian Universitas Lampung
STRUKTUR ATOM 10
M02_PETR4521_10_SE_C02.QXD 1/15/10 10:50 PM Page 45
1) Elektron.
• Partikel dalam atom yang bermuatan negative.
2) Proton.
M02_PETR4521_10_SE_C02.QXD 1/15/10 10:50 PM Page 44
• Pertikel dalam inti atom yang bermuatan positive
dan menentukan nomor atom.
3) Neutron. 2-4 Chemical Elements 45
• Partikel terdapat dalam inti, tidak bermuatan, dan
44 Chapter 2Atoms and the Atomic Theory
(bersama dengan proton) menentukan berat atom
which research team discovered a new element and, in fact, whether a discovery
TABLE 2.1 Properties of Three Fundamental Particles
was made at all. However, international agreement has been reached on the first
*The masses of the proton Electric Charge Mass
M02_PETR4521_10_SE_C02.QXD 1/15/10 10:50 PM Page 45 a
112 elements; each one, except element 112, has an official name and symbol.
and neutron are different in SI (C) Atomic SI (g) Atomic (u)
the fourth significant figure.Proton +1.6022 * 10-19 +1 1.6726 * 10-24 1.0073
The charges of the proton Neutron 0 0 -24 1.0087
andelectron, however, are 1.6749 * 10
Isotopes Electron -1.6022 * 10-19 -1 9.1094 * 10-28 0.00054858
believed to be exactly equal
in magnitude (but opposite a
u is the SI symbol for atomic mass unit (abbreviated as amu). Jurusan Teknologi Hasil Pertanian
To represent the composition of any particular atom, we need to specify its
in sign). The charges and Fakultas Pertanian Universitas Lampung
masses are known much
number of protons (p), neutrons (n), and electrons (e). We can do this with the
more precisely than suggested
here. More precise values
symbolism
are given on the inside
back cover. Properties of Protons, Neutrons, and Electrons
The number of protons in a given atom is called the atomic number, or the (2.1) 2-4 Chemical Elements 45
number p * number n A
proton number, Z. The number of electrons in the atom is also equal to Z
ZE symbol of element
number p
because the atom is electrically neutral. The total number of protons and neu-
trons in an atom is called the mass number, A. The number of neutrons, the
neutron number, is A - Z. An electron carries an atomic unit of negative
which research team discovered a new element and, in fact, whether a discovery
This symbolism indicates that the atom is element E and that it has atomic num-
charge, a proton carries an atomic unit of positive charge, and a neutron is
electrically neutral. Table 2.1 presents the charges and masses of protons, neu-
was made at all. However, international agreement has been reached on the first
ber Z and mass number A. For example, an atom of aluminum represented as
27 trons, and electrons in two ways.
The atomic mass unit(described more fully on page 46) is defined as exactly 11
Al has 13 protons and 14 neutrons in its nucleus and 13 electrons outside the
112 elements; each one, except element 112, has an official name and symbol.
13 1>12 of the mass of the atom known as carbon-12 (read as carbon twelve). An
nucleus. (Recall that an atom has the same number of electrons as protons.)
atomic mass unit is abbreviated as amu and denoted by the symbol u. As we
NOMOR ATOM, BERAT ATOM, ISOTOP
see from Table 2.1, the proton and neutron masses are just slightly greater than
Contrary to what Dalton thought, we now know that atoms of an element
Isotopes 1 u. By comparison, the mass of an electron is only about 1/2000th the mass of
1) Nomor Atom.
the proton or neutron.
do not necessarily all have the same mass. In 1912, J. J. Thomson measured
• Jumlah proton dalam inti (nucleous).
The three subatomic particles considered in this section are the only ones
To represent the composition of any particular atom, we need to specify its
involved in the phenomena of interest to us in this text. You should be aware, Because neon is the only
the mass-to-charge ratios of positive ions formed from neon atoms. From *
M02_PETR4521_10_SE_C02.QXD 1/15/10 10:50 PM Page 45
• Untuk atom netral, jumlah elektron.
however, that a study of matter at its most fundamental level must consider element with Z = 10, the
number of protons (p), neutrons (n), and electrons (e). We can do this with the
these ratios he deduced that about 91% of the atoms had one mass and that the
many additional subatomic particles. The electron is believed to be a truly fun-
2) Berat Atom. 20 21
damental particle. However, modern particle physics now considers the neu- symbols Ne, Ne, and
remaining atoms were about 10% heavier. All neon atoms have 10 protons in
symbolism tron and proton to be composed of other, more fundamental particles.
• Jumlah proton dan neutron dalam inti. 22Ne convey the same mean-
their nuclei, and most have 10 neutrons as well. Avery few neon atoms, how- 20 21 22
3) Isotop. ing as Ne, Ne, and Ne.
number p * number n (2.1) 10 10 10
ever, have 11 neutrons and some have 12. We can represent these three differ-
A
• Atom yang mempunyai nomor atom sama,
E symbol of element
2-4 Chemical Elements
ent types of neon atoms as Z
number p
beratnya berbeda.
Now that we have acquired some fundamental ideas about atomic structure, * Odd-numbered elements
we can more thoroughly discuss the concept of chemical elements.
4) Ion 20 21 22 2-4 Chemical Elements 45
All atoms of a particular element have the same atomic number, Z, and, tend to have fewer isotopes
This symbolism indicates that the atom is element E and that it has atomic num-
Ne Ne Ne
* 10 10 10
conversely, all atoms with the same number of protons are atoms of the
The discovery of element• Atom yang kehilangan atau ketambahan elektron. than do even-numbered
112 has recently been authen-same element. The elements shown on the inside front cover have atomic
ber Z and mass number A. For example, an atom of aluminum represented as
• Dapat bermuatan positive atau negative.
ticated by IUPAC. However, numbers from Z = 1 to Z = 112. Each element has a name and a distinctive elements. Section 25-7 will
27Atoms that have the same atomic number (Z) but different mass numbers (A)
which research team discovered a new element and, in fact, whether a discovery
element 112 has not yet beensymbol. Chemical symbols are one- or two-letter abbreviations of the
Al has 13 protons and 14 neutrons in its nucleus and 13 electrons outside the
13given a name or symbol. 20 explain why.
name (usually the English name). The first (but never the second) letter of
are called isotopes. Of all Ne atoms on Earth, 90.51% are Ne. The percentages
10
Jurusan Teknologi Hasil Pertanian
was made at all. However, international agreement has been reached on the first
the symbol is capitalized; for example: carbon, C; oxygen, O; neon, Ne; and
21 22 Fakultas Pertanian Universitas Lampung
nucleus. (Recall that an atom has the same number of electrons as protons.)
of Ne and Ne are 0.27% and 9.22%, respectively. These percentages
10 10 silicon, Si. Some elements known since ancient times have symbols based on
*
112 elements; each one, except element 112, has an official name and symbol.
Other atomic symbols not their Latin names, such as Fe for iron (ferrum) and Pb for lead (plumbum). The
Contrary to what Dalton thought, we now know that atoms of an element
90.51%, 0.27%, 9.22% are the percent natural abundances of the three neon
based on English names element sodium has the symbol Na, based on the Latin natrium for sodium
include Cu, Ag, Sn, Sb, Au,carbonate. Potassium has the symbol K, based on the Latin kalium for potas-
isotopes. Sometimes the mass numbers of isotopes are incorporated into the * Usually all the isotopes
do not necessarily all have the same mass. In 1912, J. J. Thomson measured
and Hg. sium carbonate. The symbol for tungsten, W, is based on the German wolfram.
Isotopes Elements beyond uranium 1Z = 922 do not occur naturally and must be of an element share the
names of elements, such as neon-20 (neon twenty). Percent natural abundances Because neon is the only
the mass-to-charge ratios of positive ions formed from neon atoms. From *
synthesized in particle accelerators (described in Chapter 25). Elements of the samename and atomic
are always based on numbers, not masses. Thus, 9051 of every 10,000 neon
very highest atomic numbers have been produced only on a limited number
To represent the composition of any particular atom, we need to specify its element with Z = 10, the
these ratios he deduced that about 91% of the atoms had one mass and that the
of occasions, a few atoms at a time. Inevitably, controversies have arisen about symbol. The exception is
atoms are neon-20 atoms. Some elements, as they exist in nature, consist of just 20 21
number of protons (p), neutrons (n), and electrons (e). We can do this with the 2 Ne, Ne,
remaining atoms were about 10% heavier. All neon atoms have 10 protons in symbols and
a single type of atom and therefore do not have naturally occurring isotopes.* hydrogen. Isotope 1H is
symbolism 22Ne convey the same mean-
called deuterium (symbol D),
their nuclei, and most have 10 neutrons as well. Avery few neon atoms, how-
Aluminum, for example, consists only of aluminum-27 atoms. 12 3 20 21 22
and His tritium (T).
1 ing as Ne, Ne, and Ne.
(2.1) 10 10 10
ever, have 11 neutrons and some have 12. We can represent these three differ-
number p * number n A y
Ions ZE symbol of element
ent types of neon atoms asnumber p
When atoms lose or gain electrons, for example, in the course of a chemical * Odd-numbered elements
This symbolism indicates that the atom is element E and that it has atomic num-
20 21 22
reaction, the species formed are called ions and carry net charges. Because an tend to have fewer isotopes
10Ne 10Ne 10Ne
ber Z and mass number A. For example, an atom of aluminum represented as
electron is negatively charged, adding electrons to an electrically neutral atom than do even-numbered
27produces a negatively charged ion. Removing electrons results in a positively
Al has 13 protons and 14 neutrons in its nucleus and 13 electrons outside the elements. Section 25-7 will
13
Atoms that have the same atomic number (Z) but different mass numbers (A)
charged ion. The number of protons does not change when an atom becomes
20
nucleus. (Recall that an atom has the same number of electrons as protons.) explain why.
are called isotopes. Of all Ne atoms on Earth, 90.51% are Ne. The percentages
20 + 22 2+ 10
21 an ion. For example, Ne and Ne are ions. The first one has 10 protons,
22
Contrary to what Dalton thought, we now know that atoms of an element
of Ne and Ne are 0.27% and 9.22%, respectively. These percentages
10 10
10 neutrons, and 9 electrons. The second one also has 10 protons, but 12 neu-
do not necessarily all have the same mass. In 1912, J. J. Thomson measured
90.51%, 0.27%, 9.22% are the percent natural abundances of the three neon
trons and 8 electrons. The charge on an ion is equal to the number of protons Because neon is the only
the mass-to-charge ratios of positive ions formed from neon atoms. From *
isotopes. Sometimes the mass numbers of isotopes are incorporated into the
minusthe number of electrons. That is * Usually all the isotopes
these ratios he deduced that about 91% of the atoms had one mass and that the element with Z = 10, the
names of elements, such as neon-20 (neon twenty). Percent natural abundances of an element share the
(2.2) 20 21
A * In this expression, #; indi-
# symbols Ne, Ne, and
remaining atoms were about 10% heavier. All neon atoms have 10 protons in
Z samename and atomic
cates that the charge is written
are always based on numbers, not masses. Thus, 9051 of every 10,000 neon 22
number p
u Neconvey the same mean-
their nuclei, and most have 10 neutrons as well. Avery few neon atoms, how-
Jurusan Teknologi Hasil Pertanian
with the number (#) before the
symbol. The exception is
Fakultas Pertanian Universitas Lampung 20 21 22
atoms are neon-20 atoms. Some elements, as they exist in nature, consist of just
16 2- ing as Ne, Ne, and Ne.
10 10 10
Another example is the O ion. In this ion, there are 8 protons (atomic 2
ever, have 11 neutrons and some have 12. We can represent these three differ- or -+ sign. However, when
a single type of atom and therefore do not have naturally occurring isotopes.* hydrogen. Isotope 1H is
number 8), 8 neutrons 1mass number - atomic number2, and 10 electrons the charge is 1+ or 1-, the
ent types of neon atoms as called deuterium (symbol D),
Aluminum, for example, consists only of aluminum-27 atoms. number 1 is not included.
18 - 10 =-22. 3
* Odd-numbered elements
20 21 22 and 1His tritium (T).
tend to have fewer isotopes
10Ne 10Ne 10Ne
Ions *Nuclide is the general term used to describe an atom with a particular atomic number and than do even-numbered
mass number. Although there are several elements with only one naturally occurring nuclide, it elements. Section 25-7 will
Atoms that have the same atomic number (Z) but different mass numbers (A)
is possible to produce additional nuclides of these elements isotopes by artificial means
When atoms lose or gain electrons, for example, in the course of a chemical
20
(Section 25-3). The artificial isotopes are radioactive, however. In all, the number of synthetic explain why.
are called isotopes. Of all Ne atoms on Earth, 90.51% are Ne. The percentages
10
reaction, the species formed are called ions and carry net charges. Because an
isotopes exceeds the number of naturally occurring ones by several fold.
of 21and 22 are 0.27% and 9.22%, respectively. These percentages
Ne Ne
10 10
electron is negatively charged, adding electrons to an electrically neutral atom
90.51%, 0.27%, 9.22% are the percent natural abundances of the three neon
produces a negatively charged ion. Removing electrons results in a positively
isotopes. Sometimes the mass numbers of isotopes are incorporated into the * Usually all the isotopes
charged ion. The number of protons does not change when an atom becomes ofan element share the
names of elements, such as neon-20 (neon twenty). Percent natural abundances
an ion. For example, 20 + and 22 2+ are ions. The first one has 10 protons,
Ne Ne samename and atomic
are always based on numbers, not masses. Thus, 9051 of every 10,000 neon
10 neutrons, and 9 electrons. The second one also has 10 protons, but 12 neu- symbol. The exception is
atoms are neon-20 atoms. Some elements, as they exist in nature, consist of just 2
trons and 8 electrons. The charge on an ion is equal to the number of protons hydrogen. Isotope 1H is
a single type of atom and therefore do not have naturally occurring isotopes.*
minusthe number of electrons. That is called deuterium (symbol D),
Aluminum, for example, consists only of aluminum-27 atoms. and 3His tritium (T).
(2.2) 1
A # * In this expression, #; indi-
Ions number p Z cates that the charge is written
When atoms lose or gain electrons, for example, in the course of a chemical with the number (#) before the
16 2-
Another example is the O ion. In this ion, there are 8 protons (atomic or -+ sign. However, when
reaction, the species formed are called ions and carry net charges. Because an
number 8), 8 neutrons 1mass number - atomic number2, and 10 electrons the charge is 1+ or 1-, the
electron is negatively charged, adding electrons to an electrically neutral atom
18 - 10 =-22. number 1 is not included.
produces a negatively charged ion. Removing electrons results in a positively
charged ion. The number of protons does not change when an atom becomes
*Nuclide is the general term used to describe an atom with a particular atomic number and
an ion. For example, 20 + and 22 2+ are ions. The first one has 10 protons,
Ne Ne
mass number. Although there are several elements with only one naturally occurring nuclide, it
10 neutrons, and 9 electrons. The second one also has 10 protons, but 12 neu-
is possible to produce additional nuclides of these elements isotopes by artificial means
trons and 8 electrons. The charge on an ion is equal to the number of protons
(Section 25-3). The artificial isotopes are radioactive, however. In all, the number of synthetic
minusthe number of electrons. That is
isotopes exceeds the number of naturally occurring ones by several fold.
A # (2.2) * In this expression, #; indi-
number p Z cates that the charge is written
16 2- with the number (#) before the
Another example is the O ion. In this ion, there are 8 protons (atomic or -+ sign. However, when
number 8), 8 neutrons 1mass number - atomic number2, and 10 electrons the charge is 1+ or 1-, the
18 - 10 =-22. number 1 is not included.
*Nuclide is the general term used to describe an atom with a particular atomic number and
mass number. Although there are several elements with only one naturally occurring nuclide, it
is possible to produce additional nuclides of these elements isotopes by artificial means
(Section 25-3). The artificial isotopes are radioactive, however. In all, the number of synthetic
isotopes exceeds the number of naturally occurring ones by several fold.
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