The Periodic Table & Trends

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The Periodic Table

Elements arranged in order of increasing atomic number.
Vertical columns are groups (numbered 1–7 and Group 0); horizontal rows are periods (numbered 1–7).
The period number equals the number of occupied electron shells.
The group number (for Groups 1–7) equals the number of outer shell electrons.
Group 0 elements have a full outer shell and are unreactive.
Metals are on the left, non-metals on the right, separated by a zig-zag line.

The Periodic Table: metals, non-metals, metalloids and liquids at room temperature

Electron Configuration & Position

Electronic configuration shows the number of electrons in each shell (e.g., carbon: 2,4).
The number of numbers in the configuration equals the period number.
The last number equals the group number (for Groups 1–7).
Example: chlorine (2,8,7) is in Period 3, Group 7.
Elements in the same group have the same number of outer electrons → similar chemical properties.

Metallic Character Trend

Metallic character decreases across a period (left to right).
Metallic character increases down a group.
Metals have 1–3 outer electrons; non-metals have 4–7 outer electrons.
Metals form basic oxides; non-metals form acidic oxides.
Metals are good conductors of electricity; non-metals are poor conductors.

The metal/non-metal divide, with basic and acidic oxide regions

Group 1 (Alkali Metals) Trends

Reactivity increases down the group (Li < Na < K < Rb < Cs < Fr).
Melting point decreases down the group.
They react with water to form a metal hydroxide and hydrogen gas.
Observations: Li fizzes slowly; Na moves rapidly; K burns with a lilac flame; Rb explodes; Cs violent explosion.

Group 7 (Halogens) Trends

Reactivity decreases down the group (F > Cl > Br > I).
Density increases down the group (F and Cl are gases, Br is liquid, I is solid at room temperature).
Halogens gain 1 electron to form ions with a 1– charge.
They are non-metals: poor conductors, brittle, low melting/boiling points.

Group 0 (Noble Gases)

All have a full outer shell of electrons (2 for He, 8 for others).
They are unreactive (inert) and exist as monatomic gases.
Used in lighting (neon signs) and as inert atmospheres (argon in welding).

Predicting Properties

Trends down groups and across periods allow prediction of melting point, boiling point, density, and reactivity.
Transition elements are denser than Group 1 elements.
Given data for a group, arrange elements in order of position to identify trends.
Francium is too reactive and rare to confirm predictions experimentally.

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1.Which one of the following names does not correspond to a group of elements on the Periodic table?
Easy
- AAlkali
- BGroup VI
- CAlloys
- DHalogens
2.Which row describes how the elements are positioned on the Periodic table and the names used?
Easy
- Aelements placed by atomic number; group = vertical column; period = horizontal row
- Belements placed by mass number; group = vertical column; period = horizontal row
- Celements placed by atomic number; group = horizontal row; period = vertical column
- Delements placed by mass number; group = horizontal row; period = vertical column
3.Which property of elements increases as you move across the Periodic table?
Easy
- AThe number of outer shells increases.
- BThe number of outer shell electrons increases.
- CThe metallic character.
- DThe tendency to become oxidised.
4.Element Z forms an ion with a 2- charge. Which group of the Periodic Table is element Z found in?
Medium
- A1
- B2
- C6
- D7
5.Element X is found in Group 7 of the Periodic Table. Which properties are typical of element X? 1. Poor conductor of electricity 2. Malleable 3. High melting points 4. Form acidic oxides
Medium
- A1 and 2
- B1 and 4
- C2 and 3
- D3 and 4
6.The table shows the densities at room temperature of halogens W, X, Y and Z: W 0.0017 g/cm3, X 3.1 g/cm3, Y 0.0032 g/cm3, Z 4.93 g/cm3. Which row correctly identifies W, X, Y and Z?
Medium
- AW=fluorine, X=chlorine, Y=bromine, Z=iodine
- BW=fluorine, X=bromine, Y=chlorine, Z=iodine
- CW=iodine, X=chlorine, Y=bromine, Z=fluorine
- DW=iodine, X=bromine, Y=chlorine, Z=fluorine
7.Potassium and krypton are elements in Period 4. Potassium is at the beginning of the period and is more metallic than krypton which is at the end of the period. What makes potassium more metallic than krypton?
Medium
- AIt has less electrons than krypton.
- BIt has less protons than krypton.
- CIt has less electron shells.
- DIt has less outer shell electrons.
8.The elements of the Periodic table can be broadly classified into metals and nonmetals. Which statements are correct? 1. Magnesium is more metallic than silicon. 2. Boron is more metallic than lithium. 3. Carbon is less metallic than beryllium. 4. Sodium is less metallic than aluminium.
Hard
- A1 and 3
- B1 and 2
- C2, 3 and 4
- D1, 2 and 4

Plus de questions

9.An element has an electronic configuration of 2,8,6. Which group and period can the element be found in?
Medium
- AGroup 6, Period 3
- BGroup 6, Period 8
- CGroup 3, Period 6
- DGroup 8, Period 2
10.Potassium has a lower relative atomic mass than argon but on the Periodic table potassium appears after argon. Why is potassium placed after argon?
Medium
- AArgon has less neutrons than potassium.
- BArgon has more protons than potassium.
- CPotassium has more protons than argon.
- DPotassium has more neutrons than argon.
11.Oxygen, sulfur, selenium and tellurium are Group VI elements. What do all these elements have in common?
Medium
- AThey all have 6 outer shell electrons and have similar physical properties.
- BThey are all non-metals.
- CThey all have 5 outer shell electrons and have similar chemical properties.
- DThey all have 6 outer shell electrons and have similar chemical properties.
12.As you move down a group on the Periodic table the elements become more metallic in character. Which statement explains this observation?
Medium
- AElectrons are more easily gained due to increasing atomic radius.
- BElectrons are more easily lost due to increasing atomic radius.
- CThe elements are heavier due to the atomic number increasing as you move down a group.
- DThe elements are heavier due to the mass number increasing as you move down a group.
13.The table shows the melting points of the Group 1 metals lithium, sodium and potassium. Lithium melts at 180°C, sodium at 98°C, and potassium at 63°C. What is the general trend in melting points as you go down Group 1?
Easy
- AMelting point decreases
- BMelting point increases
- CMelting point stays the same
- DMelting point first increases then decreases
14.The table shows the boiling points of the halogens at room temperature: fluorine -188°C, chlorine -34°C, bromine 59°C, iodine 184°C. What is the trend in boiling points as you go down Group 7?
Easy
- ABoiling point increases
- BBoiling point decreases
- CBoiling point stays the same
- DBoiling point first increases then decreases
15.An element X has an electronic configuration of 2,8,3. It forms an oxide. What is the formula of the oxide of X?
Medium
- AX2O3
- BXO2
- CX2O
- DXO
16.Element Y is in Group 6 and Period 3. What is the electronic configuration of Y?
Medium
- A2,8,6
- B2,6
- C2,8,4
- D2,8,8,6
17.The table gives the atomic radii (in pm) of some elements in Period 3: Na 186, Mg 160, Al 143, Si 117, P 110, S 104, Cl 99. What is the trend in atomic radius across Period 3?
Easy
- AAtomic radius decreases
- BAtomic radius increases
- CAtomic radius stays the same
- DAtomic radius first decreases then increases
18.Which statement explains why atomic radius decreases across a period?
Medium
- AIncreasing nuclear charge pulls electrons closer
- BMore electron shells are added
- CElectrons are lost from the outer shell
- DThe number of neutrons increases
19.Element Z is a metal in Group 2. It reacts with chlorine to form a compound. What is the formula of the compound formed?
Medium
- AZCl2
- BZCl
- CZ2Cl
- DZCl3
20.The table shows the first ionization energies (kJ/mol) of elements in Period 2: Li 520, Be 900, B 801, C 1086, N 1402, O 1314, F 1681, Ne 2081. Which element has the highest first ionization energy?
Easy
- ANeon
- BLithium
- CFluorine
- DNitrogen
21.Which of the following statements about the reactivity of Group 7 elements is correct?
Easy
- AReactivity decreases down the group
- BReactivity increases down the group
- CReactivity remains the same down the group
- DReactivity first increases then decreases down the group
22.Which element is in Group 7 and Period 3?
Easy
- AChlorine
- BFluorine
- CBromine
- DIodine
23.Which element has the electronic configuration 2,8,2?
Easy
- AMagnesium
- BCalcium
- CSodium
- DAluminium
24.In an experiment, a student adds a small piece of lithium to water in a trough. Which observation would the student NOT see?
Medium
- AThe lithium fizzes and moves on the surface.
- BA lilac flame is produced.
- CThe lithium dissolves slowly.
- DHydrogen gas is evolved.
25.A student is given four unlabelled samples of Group 1 metals: lithium, sodium, potassium, and rubidium. She places a small piece of each in separate troughs of water and records the observations. Which metal would produce a violent explosion with sparks?
Easy
- ALithium
- BSodium
- CPotassium
- DRubidium
26.The table shows the melting points of some Group 1 metals: lithium 180°C, sodium 98°C, potassium 63°C, rubidium 39°C. What is the predicted melting point of caesium?
Medium
- A28°C
- B45°C
- C55°C
- D72°C
27.An element X has the electronic configuration 2,8,8,2. Which statements about X are correct? 1. It is in Group 2. 2. It is in Period 4. 3. It forms an ion with a 2+ charge. 4. It is a non-metal.
Medium
- A1, 2 and 3
- B1 and 2
- C2 and 4
- D1, 2, 3 and 4
28.Which of the following is a property of non-metals?
Easy
- AThey are good conductors of electricity.
- BThey are malleable.
- CThey form basic oxides.
- DThey have low melting and boiling points.
29.An element Y has an electronic configuration of 2,8,7. Which group and period is Y in?
Easy
- AGroup 7, Period 2
- BGroup 7, Period 3
- CGroup 5, Period 2
- DGroup 5, Period 3
30.The atomic radii (in pm) of some Period 3 elements are: Na 186, Mg 160, Al 143, Si 117, P 110, S 104, Cl 99. Which statement explains the trend in atomic radius across Period 3?
Medium
- AThe number of electron shells increases.
- BThe nuclear charge increases, pulling the electrons closer.
- CThe number of outer electrons decreases.
- DThe shielding effect increases.
31.Which of the following elements is a metalloid?
Easy
- ASodium
- BSilicon
- CChlorine
- DArgon
32.Which element is unreactive and found in Group 0?
Easy
- ANeon
- BChlorine
- CSodium
- DOxygen
33.The first ionization energies (kJ/mol) of Period 2 elements are: Li 520, Be 900, B 801, C 1086, N 1402, O 1314, F 1681, Ne 2081. Which element has the highest first ionization energy?
Easy
- ALithium
- BNitrogen
- COxygen
- DNeon
34.An element Z is in Group 6 and Period 2. What is the formula of the ion it forms?
Medium
- AZ2+
- BZ2-
- CZ6+
- DZ6-
35.The table shows the boiling points of the halogens: fluorine -188°C, chlorine -34°C, bromine 59°C, iodine 184°C. Which statement about the trend in boiling point is correct?
Easy
- ABoiling point decreases down the group.
- BBoiling point increases down the group.
- CBoiling point is highest for fluorine.
- DBoiling point is lowest for iodine.
36.What is the order of increasing atomic number used for in the Periodic Table?
Easy
- ATo arrange elements in order of increasing atomic mass
- BTo arrange elements in order of increasing atomic number
- CTo arrange elements in order of increasing number of neutrons
- DTo arrange elements in order of increasing number of protons and neutrons
37.Which of the following elements is unreactive?
Easy
- ANe
- BLi
- CO
- DCa
38.What does the period number of an element tell you?
Easy
- AThe number of outer shell electrons
- BThe number of electron shells
- CThe number of protons
- DThe number of neutrons
39.Which statement about the metallic character of elements is correct?
Medium
- AMetallic character increases across a period and decreases down a group
- BMetallic character decreases across a period and increases down a group
- CMetallic character increases across a period and increases down a group
- DMetallic character decreases across a period and decreases down a group
40.Elements are arranged on the Periodic Table in order of increasing atomic mass.
Easy
True or false?
41.An element has the electronic configuration 2,8,2. Which group is it in?
Easy
- AGroup 2
- BGroup 8
- CGroup 12
- DGroup 0
42.Group 0 elements are also known as the noble gases.
Easy
True or false?
43.Which statement about the reactivity of Group 1 metals is correct?
Easy
- AReactivity decreases down the group
- BReactivity increases down the group
- CReactivity stays the same down the group
- DReactivity is unpredictable
44.Which of the following are properties of metals? (Select all that apply)
Medium
- AGood conductors of electricity
- BBrittle
- CMalleable
- DForm basic oxides
- EForm acidic oxides
45.Arrange the following Group 1 elements in order of increasing reactivity: lithium, sodium, potassium, rubidium.
Easy
- lithium
- sodium
- potassium
- rubidium
46.Across a period from left to right, metallic character increases.
Easy
True or false?
47.Match each element to its correct group based on the number of outer electrons.
Medium
- Element with 1 outer electron
- Element with 4 outer electrons
- Element with 7 outer electrons
- Element with 8 outer electrons
- Group 1
- Group 4
- Group 7
- Group 0
48.Arrange the following Group 1 metals in order of increasing reactivity with water: lithium, potassium, sodium, rubidium.
Easy
- lithium
- sodium
- potassium
- rubidium
49.Which of the following are properties of non-metals? (Select all that apply)
Medium
- AGood conductors of electricity
- BBrittle
- CForm acidic oxides
- DMalleable
- ELow melting and boiling points
50.Complete the sentence using the correct terms.
Easy
The vertical columns on the Periodic Table are called ____ and the horizontal rows are called ____.
51.What is the term for elements that display some properties of both metals and non-metals?
Easy
52.Fill in the blanks to complete the sentence about periodic trends.
Medium
Across a period, metallic character ____. Down a group, metallic character ____.
53.An element has electronic configuration 2,8,6. What is its atomic number?
Easy
54.Explain why elements in the same group have similar chemical properties.
Medium
55.An element has electronic configuration 2,8,6. What is its atomic number?
Easy
- A18
- B16
- C15
- D17

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