LESSON 1: Basic Chemistry |
Atoms & Ions | Chemical Bonding | Water | Acid & Bases | Organic Compounds | Carbohydrates | Lipids | Proteins | Enzymes | Nucleic Acids | ATP |
168+9 sentence examples: 1. The nucleus of an atom consists of neutrons, protons and other particles. Two atoms of hydrogen combine with one atom of oxygen to form a molecule of water. The particles in an atom are infinitely small. Examples of chemical species that are not typically considered atoms includes particles that are components of atoms: protons, neutrons, and electrons. Molecules and compounds consist of atoms but are not themselves atoms. Examples of molecules and compounds include salt (NaCl), water (H 2 O) and methanol (CH 2 OH). Example: Find the number of protons of atom having mass number 65 and neutron number 35. Mass number is equal to sum of protons and neutrons. Example: Which ones of the following statements are true for 12 24 X and 11 24 Y atoms. Number of protons XY. Neutron number of Y is larger than neutron number of X. You just inhaled trillions of atoms of nitrogen and oxygen, as well as some other gases. Go get a drink of water. You just ingested trillions of atoms of hydrogen and oxygen, with some others mixed in, like chlorine and fluorine, various minerals dissolved in the water. For example, the language-html package that provides support for HTML syntax highlighting and grammar comes with dozens of snippets to create many of the various HTML tags you might want to use. If you create a new HTML file in Atom, you can type html and then press Tab and it will expand to.
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ATOMS AND IONS
Atoms
Atoms are the basic unit of chemistry. They consist of 3 smaller things:
- Protons - these are positively charged (+)
- Electrons - these are negatively charged (-)
- Neutrons - these have no charge
These 3 smaller particles are arranged in a particular way. In the center is the Nucleus where you find the positive Protons and neutral Neutrons.
In orbit around the nucleus are the Electrons. These are found in a series of orbits (depending on the atom) with differing numbers of electrons as seen below.
Interaction of Atoms
Discrete Atom Examples
It's the electrons in orbit around the nucleus that allow one atom to interact with other atoms so they can be linked together.
For example, H2O consists of an Oxygen atom linked to 2 Hydrogen atoms. The linkage or interaction between the electrons of the Hydrogen and Oxygen atoms is called a Chemical Bond. More on these later.
Atoms in the Human Body
The human body is made up of a couple dollars worth of chemicals.
The 12 most useful atoms for you to know about are listed below:
Ions
Sometimes atoms gain or lose electrons. The atom then loses or gains a 'negative' charge. These atoms are then called ions.
- Positive Ion - Occurs when an atom loses an electron (negative charge) it has more protons than electrons.
- Negative Ion - Occurs when an atom gains an electron (negative charge) it will have more electrons than protons.
The following image shows Na losing an electron and Cl gaining an electron
- Thus the Na becomes Na+
- The Cl becomes Cl-
Here are some examples of common ions: | |
Na+ | Sodium |
K+ | Potassium |
Cl- | Chloride |
Ca+ | Calcium |
Fe+ | Iron |
P- | Phosphorous |
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Atomic Structure with Examples
Atomic Structure with Examples
Atom is the smallest particle of matter. It consist of three particles, called proton, electron and neutron. Protons and neutrons are placed at the center of the atom and electrons are placed around the center. Picture given below shows, structure of atom and locations of proton neutron and electron in atom.
Center of the atom, including protons and neutrons, is called also nucleus and circles around nucleus are called orbits.
Protons: Protons are positively charged particles of atoms. They are located in nucleus, and have mass. We show protons with letter 'p'.
Electrons: Electrons are negatively charged moving particles of atoms. They are located around the nucleus on orbits, and have no mass. We show electrons with letter 'e'.
Neutrons: Neutrons are charge-less particles of atoms. They are located in nucleus, and have mass. We show neutrons with letter 'n'.
Atomic Number:
Atomic number shows the number of protons in each atom. It is specific for each atom and shown with letter 'Z'. In neutral atom number of protons is equal to number of electrons. Thus;
Z=p=e
Atomic number is written as;
atomic numberX
Mass Number:
Mass of the neutron is approximately equal to the mass of proton. We neglect mass of electron since it is too small. Thus, mass of atom is equal to the sum of mass of protons and neutrons. We show mass number with letter 'M'. Mass number is not specific for each atom. Different atoms can have same mass number.
M=n+p
We show M on atom as;
ZMX
Isotopes:
Isotopes have same atomic number but different mass number. This means that atoms have same number of protons but different number of neutrons. Since the number of protons are equal, chemical properties of the atoms are same, and since the neutrons numbers are different physical properties of atoms are different. Isotopes of Hydrogen are given below;
11H,
12H ,
13H
Isotones:
Isotone atoms have same number of neutrons and different numbers of protons.
Sodium and Magnesium are isotone atoms, their numbers of neutrons are equal.
1123Na and 1224Mg
Isobars:
Isobar atoms have different atomic number and different neutron number but same mass number.
1124Na and 1224Mg
Since the protons number and neutrons number of atoms are different, their physical and chemical properties are also different.
Example: Which one of the following statements are same for isotope atoms
I. Number of protons
II. Number of neutrons
III. Number of electrons
IV. Atomic Number
Examples Of Atomic Solids
V. Chemical properties
VI. Physical Properties
Isotopes have same atomic number bur different mass number. This means that, isotopes atoms have equal number of protons and different number of neutrons. If the atom is neutral then number of protons in the atom is equal yo number of electrons. Since the number of protons of atoms are equal and number of neutrons are different; chemical properties of these atoms are same but physical properties of them are different. Thus;
I. How to clear your phone storage recovery. III. IV. and V is true for isotopes atoms.
Example: Find the number of protons of atom having mass number 65 and neutron number 35.
Mass number is equal to sum of protons and neutrons.
M=p+n
65=35+p
p=30
Example: Which ones of the following statements are true for 1224X and 1124Y atoms.
I. Number of protons X>Y
II. neutron number of Y is larger than neutron number of X
III. Their mass numbers are equal
1224X :
X has 12 protons and
24-12=12 neutrons
Mass number=24
124Y:
Y has 11 protons and
24-11=13 neutrons
Mass number=24
Thus, I. II. and III. are true.
Example:
I. 2656Fe+2, 2656Fe+3
II. 2656Fe, 2756Co
III. H2O, D2O
Which one of the couples given above has same chemical properties. (11H, 12D)
To have same chemical properties, they must have equal numbers of protons and electrons.
I. Both of them has same numbers of proton 26, but their electron numbers are different. First one has 26-2=24 electrons and second one has 26-3=23 electrons. Thus they have different chemical properties.
Atom Examples Chemistry
II. Since both of them have different numbers of protons and electrons, they have different chemical properties.
Repeating Groups Of Atom Examples
III. In this couple, they have equal number of protons and electrons they have same chemical properties.
Next >Electron Configuration with Examples |
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Simple Explanation Of An Atom
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