The Periodic Table (Edexcel IGCSE Chemistry (Modular): Unit 1): Flashcards
Exam code: 4XCH1
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What is a period in the Periodic Table?
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What is a period in the Periodic Table?
A period is a horizontal row of the Periodic Table. The period number indicates how many electron shells an atom of that element has.
What is a group in the Periodic Table?
A group is a vertical column of the Periodic Table. The group number indicates how many outer electrons an atom has in its outermost shell.
How are elements arranged in the Periodic Table?
Elements are arranged in order of increasing atomic number. Each element has one more proton than the element before it.
True or False?
All elements in Group 4 have 4 electrons in their outer shell.
True.
The group number directly indicates the number of outer shell electrons for elements in that group. Group 4 elements each have 4 electrons in their outermost shell.
Elements in the Periodic Table are arranged in vertical columns called .......... and in horizontal rows called ...........
Elements in the Periodic Table are arranged in vertical columns called groups and in horizontal rows called periods.
How does the period number of an element relate to its electron shells?
The period number tells you the number of electron shells in an atom of that element. For example, elements in Period 3 have three electron shells.
True or False?
The last group on the Periodic Table is called Group 8.
False.
The last group is called Group 0 (not Group 8). It contains the noble gases, which have full outer electron shells.
What is the electronic configuration of an atom?
Electronic configuration describes the arrangement of electrons in an atom's shells, written as numbers separated by commas showing how many electrons occupy each shell.
How many electrons can each of the first three shells hold?
The first shell holds a maximum of 2 electrons, the second shell holds a maximum of 8, and the third shell holds a maximum of 8 (using the simplified IGCSE model).
Electrons fill the .......... closest to the nucleus first. When a shell becomes full, electrons start to fill the .......... shell.
Electrons fill the shell closest to the nucleus first. When a shell becomes full, electrons start to fill the next shell.
True or False?
The electronic configuration of sodium (atomic number 11) is 2, 8, 1.
True.
Sodium has 11 electrons: 2 in the first shell, 8 in the second, and 1 in the third. Its electronic configuration is 2, 8, 1.
Complete the electronic configurations for these elements.
Element
Atomic Number
Electronic Configuration
Lithium
3
Carbon
6
Neon
10
Chlorine
17
Potassium
19
Element
Atomic Number
Electronic Configuration
Lithium
3
2, 1
Carbon
6
2, 4
Neon
10
2, 8
Chlorine
17
2, 8, 7
Potassium
19
2, 8, 8, 1
What does the number of notations in an electronic configuration tell you about an element?
The number of notations tells you how many electron shells are occupied, which gives the element's period in the Periodic Table.
True or False?
Elements in the same group of the Periodic Table have the same number of electron shells.
False.
Elements in the same group have the same number of outer electrons, not the same number of shells. Elements in the same period share the same number of electron shells.
Chlorine has the electronic configuration 2, 8, 7. In which period and group is chlorine?
Chlorine has 3 notations, so it is in Period 3. Its last notation is 7, so it has 7 outer electrons and belongs to Group 7.
What is an electron shell?
An electron shell is a region around the nucleus where electrons are found. Shells are also called energy levels; shells further from the nucleus have more energy.
What does the last notation in an electronic configuration reveal about an element?
The last notation reveals the number of electrons in the outermost shell, which determines which group the element belongs to in the Periodic Table.
Where are metals and non-metals located in the Periodic Table?
Metals are found on the left side of the Periodic Table and non-metals are on the right. They are separated by a zig-zag line.
What is a metalloid (semi-metal)?
A metalloid (also called a semi-metal) is an element that lies along the zig-zag line dividing metals and non-metals in the Periodic Table. Metalloids have characteristics of both metals and non-metals.
True or False?
Non-metals are good conductors of electricity.
False.
Non-metals are generally poor conductors of electricity. It is metals that are good conductors.
Complete the table comparing properties of metals and non-metals.
Property
Metals
Non-metals
Electrical conductivity
Type of oxide
Physical state at room temperature
Property
Metals
Non-metals
Electrical conductivity
Good conductor
Poor conductor
Type of oxide
Basic
Acidic
Physical state at room temperature
Mostly solid
Variable (solid, liquid, or gas)
What type of oxides do metals and non-metals typically form?
Metals typically form basic oxides, while non-metals typically form acidic oxides (though some non-metal oxides are neutral).
True or False?
Metals are usually malleable and have high melting points.
True.
Metals are typically malleable (can be bent and shaped) and have high melting and boiling points. Most are solid at room temperature — mercury is the main exception.
Metals typically have .......... to 3 outer shell electrons and form .......... bonds, while non-metals have 4 to .......... outer shell electrons and bond covalently.
Metals typically have 1 to 3 outer shell electrons and form metallic bonds, while non-metals have 4 to 7 outer shell electrons and bond covalently.
How can electrical conductivity be used to classify an element as a metal or non-metal?
Metals are good conductors of electricity, while non-metals are generally poor conductors. Testing electrical conductivity is therefore a useful way to classify an unknown element.
What are basic oxides?
Basic oxides are oxides formed by metals. They contrast with acidic oxides, which are typically formed by non-metals.
Why do elements in the same group have similar chemical properties?
Elements in the same group all have the same number of outer electrons. Since outer electrons control how an element reacts and bonds, elements in the same group behave similarly.
What are noble gases?
Noble gases are the elements in Group 0 of the Periodic Table. They are non-metals that exist as single (monatomic) atoms and are colourless, non-flammable gases at room temperature.
True or False?
Noble gases are unreactive because they have no electrons.
False.
Noble gases are unreactive because they have full outer electron shells. Most have 8 outer electrons (helium has 2), so they have no need to lose, gain, or share electrons.
Noble gases are described as .......... because they have .......... outer electron shells and do not easily form ...........
Noble gases are described as inert because they have full outer electron shells and do not easily form molecules.
How does reactivity change as you move down Group 1?
Group 1 elements become more reactive as you move down the group. For example, potassium is more reactive than sodium, which is more reactive than lithium.
True or False?
All noble gases have 8 electrons in their outer shell.
False.
Most noble gases have 8 outer electrons, but helium is the exception — it has only 2, because its first shell can hold a maximum of 2 electrons.
Complete the electronic configurations for these noble gases.
Noble Gas
Electronic Configuration
Helium (He)
Neon (Ne)
2, 8
Argon (Ar)
Krypton (Kr)
2, 8, 18, 8
Xenon (Xe)
Noble Gas
Electronic Configuration
Helium (He)
2
Neon (Ne)
2, 8
Argon (Ar)
2, 8, 8
Krypton (Kr)
2, 8, 18, 8
Xenon (Xe)
2, 8, 18, 18, 8
How does reactivity change as you move down Group 7?
Group 7 elements become less reactive as you move down the group. This is the opposite trend to Group 1, where reactivity increases going down.
What does monatomic mean?
Monatomic describes a substance that exists as single, individual atoms rather than bonded into molecules. The noble gases are monatomic.
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