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WorksheetsYear 10 Science- Semester 1- Exam revision- Periodic Table
Total questions: 68
Worksheet time: 34mins
Name the particles in the nucleus.
Protons and neutrons
Electrons and protons
Neutrons and electrons
Quarks and electrons
Name the particles in the space around the nucleus.
Electrons
Protons
Neutrons
Quarks
List the following in order from smallest to largest: atom, electron, proton, neutron.
Electron, proton, neutron, atom
Atom, electron, proton, neutron
Proton, electron, neutron, atom
Neutron, proton, electron, atom
A particular atom has 8 protons, 8 electrons and 9 neutrons. State its atomic number.
8
9
16
1
State the element symbol for oxygen.
O
Ox
Og
Oy
State the element symbol for chlorine.
Cl
Ch
Cn
Co
State the element symbol for magnesium.
Mg
Mn
Ma
Mg2
State the element symbol for iron.
Fe
Ir
In
I
Name the following element: F.
Fluorine
Francium
Iron
Phosphorus
Name the following element: Ca.
Calcium
Carbon
Cadmium
Chlorine
Name the following element: Na.
Sodium
Potassium
Calcium
Magnesium
Name the following element: Pb.
Lead
Platinum
Phosphorus
Palladium
State the electric charge of a proton.
Positive (+1)
Negative (-1)
Neutral (0)
Double positive (+2)
State the electric charge of an electron.
Negative (-1)
Positive (+1)
Zero (0)
Positive (+2)
State the electric charge of a neutron.
Neutral (0)
Positive (+1)
Negative (-1)
Positive (+2)
State the electric charge of a nucleus.
Positive (due to protons)
Negative (due to electrons)
Neutral (no charge)
Variable (depends on atom)
State the electric charge of an atom.
Neutral (0)
Positive (+)
Negative (-)
Double positive (++)
State the number of electrons that can fit in each of the first four electron shells. (using 2n2 method)
2, 8, 18, 32
2, 8, 8, 18
2, 4, 8, 16
2, 6, 10, 14
State how many electrons are in an atom that has an electron configuration of 2,8,8.
18
16
20
10
Define the following term: atomic number.
The number of protons in the nucleus of an atom.
The number of neutrons in the nucleus of an atom.
The total number of electrons in an atom.
The sum of protons and neutrons in the nucleus of an atom.
Explain why most of an atom's mass is due to its nucleus.
Most of an atom's mass is due to its nucleus because the nucleus contains protons and neutrons, which are much heavier than electrons.
Most of an atom's mass is due to its nucleus because electrons are heavier than protons and neutrons.
Most of an atom's mass is due to its nucleus because the nucleus contains only electrons.
Most of an atom's mass is due to its nucleus because the nucleus is made up of empty space.
Use the formula 2n2 to calculate the maximum number of electrons held by shell 5 (n = 5 ).
The maximum number of electrons held by shell 5 is 50.
The maximum number of electrons held by shell 5 is 40.
The maximum number of electrons held by shell 5 is 32.
The maximum number of electrons held by shell 5 is 20.
Identify the type of atoms and the number of each type in a single molecule of: a. methane, CH4 b. nitric acid, HNO3 c. glucose, C6H12O6 d. ethanoic acid (vinegar), CH3COOH.
a. 1 carbon, 4 hydrogen b. 1 hydrogen, 1 nitrogen, 3 oxygen c. 6 carbon, 12 hydrogen, 6 oxygen d. 2 carbon, 4 hydrogen, 2 oxygen
a. 1 carbon, 2 hydrogen b. 1 hydrogen, 2 nitrogen, 3 oxygen c. 6 carbon, 6 hydrogen, 12 oxygen d. 2 carbon, 2 hydrogen, 4 oxygen
a. 2 carbon, 4 hydrogen b. 1 hydrogen, 1 nitrogen, 2 oxygen c. 12 carbon, 6 hydrogen, 6 oxygen d. 1 carbon, 4 hydrogen, 2 oxygen
a. 1 carbon, 3 hydrogen b. 2 hydrogen, 1 nitrogen, 3 oxygen c. 6 carbon, 12 hydrogen, 12 oxygen d. 2 carbon, 4 hydrogen, 1 oxygen
Which of the following correctly compares a proton and a neutron?
Both have the same mass and no charge.
Proton is positively charged, neutron has no charge; both have similar mass.
Proton is negatively charged, neutron is positively charged.
Both have different masses and both are positively charged.
An atom of aluminium differs from an atom of carbon in that aluminium has:
fewer protons than carbon
the same number of protons as carbon
more protons than carbon
no protons
A subatomic particle is:
A particle smaller than an atom
A type of chemical bond
A large molecule
A form of energy
Which of the following is a way to remember element symbols that don't seem to match their names?
Create mnemonics linking the symbol to the element's Latin name.
Ignore the symbols and use only the names.
Memorize the periodic table in alphabetical order.
Use only the first letter of each element.
List five group 15 elements.
Nitrogen, phosphorus, arsenic, antimony, bismuth.
Hydrogen, helium, lithium, beryllium, boron.
Oxygen, sulfur, selenium, tellurium, polonium.
Fluorine, chlorine, bromine, iodine, astatine.
List five period 2 elements.
Lithium, beryllium, boron, carbon, nitrogen.
Sodium, magnesium, aluminum, silicon, phosphorus.
Potassium, calcium, scandium, titanium, vanadium.
Helium, neon, argon, krypton, xenon.
List five common transition elements.
Iron, copper, zinc, nickel, chromium.
Sodium, potassium, calcium, magnesium, lithium.
Helium, neon, argon, krypton, xenon.
Carbon, hydrogen, oxygen, nitrogen, sulfur.
List five lanthanides.
Lanthanum, cerium, praseodymium, neodymium, samarium.
Sodium, magnesium, aluminum, silicon, phosphorus.
Iron, copper, zinc, silver, gold.
Helium, neon, argon, krypton, xenon.
List five actinides.
Actinium, thorium, uranium, plutonium, americium.
Sodium, potassium, calcium, magnesium, lithium.
Helium, neon, argon, krypton, xenon.
Iron, copper, zinc, silver, gold.
The electron configuration of an element determines its position in the periodic table by:
Indicating its group and period based on the number of valence electrons and energy levels.
Showing the atomic mass of the element.
Determining the color of the element.
Predicting the melting point of the element.
The electron configurations of an element is given below. Identify in which period and group they should be placed.
(2, 3)
Period 2, Group 3
Period 3, Group 2
Period 4, Group 1
Period 2, Group 5
The electron configurations of different elements are given below. Identify in which period and group they should be placed. b 2,8,7
Period 3, Group 17
Period 2, Group 16
Period 4, Group 15
Period 3, Group 16
The electron configurations of different elements are given below. Identify in which period and group they should be placed. c 2,8,8,2
Period 4, Group 2
Period 3, Group 2
Period 4, Group 1
Period 2, Group 2
The electron configuration of an element is given below. Identify in which period and group they should be placed.
(2,8,7)
Period 4, Group 16
Period 3, Group 17
Period 2, Group 15
Period 5, Group 14
Use the periodic table to help you predict the electron configuration for: a silicon (Si)
2,8,4
2,8,8
2,4,8
2,6,6
Use the periodic table to help you predict the electron configuration for: b helium (He)
2
2, 1
2, 1, 1
1
Use the periodic table to help you predict the electron configuration for: c nitrogen (N)
2,5
2,6
2,8
2,7
Use the periodic table to help you predict the electron configuration for: d magnesium (Mg)
2,8,2
2,8,8,2
2,2,8
2,8,4
Identify the period and group that these atoms would belong to. a Ne
Period 2, Group 18
Period 3, Group 17
Period 1, Group 1
Period 2, Group 2
Identify the period and group that these atoms would belong to. b an atom with atomic number 13
Period 3, Group 13
Period 2, Group 2
Period 4, Group 1
Period 3, Group 2
Use the periodic table to determine the electron configuration of an atom in: a period 2, group 16
2,6
2,8
2,4
2,2
Use the periodic table to determine the electron configuration of an atom in: b period 3, group 18.
2,8,8
2,8,7
2,8,6
2,8,2
Use the periodic table to determine how many electrons in an atom: a with eight protons
8
6
10
12
Use the periodic table to determine how many electrons in an atom: b with 18 protons
18
8
20
16
Use the periodic table to determine how many electrons in an atom: c with an atomic number of 3
3
6
1
12
Use the periodic table to determine how many electrons in an atom: d with an atomic number of 19
19
18
20
17
Use the periodic table to determine how many electrons in an atom: e in period 2, group 17
9
7
8
10
Use the periodic table to determine how many electrons in an atom: f in period 3, group 2
12
10
14
8
Use the periodic table to determine how many electrons in an atom: g of phosphorus
15
16
14
18
Use the periodic table to determine how many electrons in an atom: h of potassium.
19
18
20
17
Which of the following statements correctly compares the elements H, Li, and Na in terms of their electron configurations and placement in the periodic table?
All three elements are in the same group and have similar valence electron configurations.
H and Li are in the same group, but Na is in a different group.
Li and Na are in the same group and have similar valence electron configurations, while H is in a different group.
All three elements have completely different electron configurations and are in different groups.
Name an element that has similar properties to: Oxygen.
Sulfur
Sodium
Iron
Chlorine
State the chemical formulas for molecules of fluorine and molecules of chlorine.
F2 and Cl2
F and Cl
F2 and Cl
F and Cl2
Helium is used instead of hydrogen in airships because:
Helium is less dense than hydrogen
Helium is more flammable than hydrogen
Helium is non-flammable, unlike hydrogen
Helium is heavier than hydrogen
Oxygen and sulfur form similar molecules such as H2O and H2S because they have similar electron configurations. Which of the following best explains this similarity?
Both have six valence electrons and belong to the same group in the periodic table.
Both have completely filled outer shells.
Both are metals with similar properties.
Both have the same atomic number.
Contrast these two groups.
Noble gases and halogens
They are similar in all aspects.
They have different characteristics.
They belong to the same category.
They have the same function.
Which of the following correctly compares the similarities and differences between alkali metals and alkaline earth metals?
Both are highly reactive, but alkali metals are more reactive and have one valence electron, while alkaline earth metals have two.
Both are non-metals and have similar reactivity.
Alkali metals are less reactive than alkaline earth metals and both have two valence electrons.
Both groups are found in the p-block of the periodic table.
Propose a reason why helium is the best noble gas for use in party balloons.
It is lighter than air and non-flammable.
It is heavier than air and flammable.
It reacts easily with other gases.
It is toxic to humans.
10. Tin acts like a non-metal below 13°C. In 1913 Captain Robert Scott and two fellow explorers froze to death in Antarctica after they ran out of heating fuel that was stored in tins. The most likely reason they unexpectedly ran out of fuel is:
Tin became brittle and cracked, causing the tins to leak fuel.
Tin became magnetic and attracted the fuel away.
Tin reacted with the fuel and neutralized it.
Tin turned into a gas and evaporated.
State which of the following is the correct symbol for sodium.
So
Sm
Na
NA
State which of the following statements is incorrect.
Chlorine is in period 3.
Chlorine is in group 17.
Chlorine has the atomic number 17.
Chlorine would react in a similar way to O, N, C and B.
Every new period represents another electron shell being added to an atom. From this information, identify the statement below that is definitely true.
Helium is the biggest of all the group 18 elements.
A sulfur atom is bigger than an oxygen atom.
A sulfur atom is bigger than a phosphorus atom.
A sodium atom is bigger than a potassium atom.
Atoms in the same group of a periodic table tend to form similar molecules. Carbon and chlorine form the molecule CCl4. Use this information and the periodic table to identify which of the following molecules could not occur.
CN4
CBr4
CF4
SiCl4
Which of the following elements is a noble gas?
Neon
Oxygen
Nitrogen
Chlorine
State the element symbol for iron.
Io
In
Ir
Fe
