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C1 Atomic Structure and Periodic Table

Last updated about 1 month ago
226 questions
4.1.1.1 Atoms, Elements, and compounds
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Give the element symbol for the following elements.
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Copper

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Fluorine

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Gallium

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Hydrogen

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Indium

Give the element name that matches the symbol below.
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Au

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Ge

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I (This is a capital "i")

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He

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W

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What do we call a substance that cannot be broken down into simpler substances by chemical means?

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Which term describes a substance composed of two or more elements that are chemically combined?

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Made up of 2 or more different atoms bonded together.

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Two or more atoms bonded together.

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How many atoms make up this compound?

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How many atoms of oxygen are there in Hâ‚‚Oâ‚‚

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What is the correct name for NaCl?

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What is the chemical name for the compound CaO?

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The correct name for the compound KBr is?

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What is the correct name for the compound MgBr2?

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What is the correct name for the compound Al2S3?

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Other Answer Choices:
molecule
atom
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Other Answer Choices:
Not an element
Element
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Other Answer Choices:
Molecule
Element
Both!
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Other Answer Choices:
Both!
Compound
Molecule
4.1.1.2 Mixtures
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Tom mixed sand and water together for a science experiment. What is this combination called?

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Which method is used to separate based on boiling point?

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What is the process used to separate crystals?

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Which technique is best for separating colored pigments in a substance?

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What method is utilized to remove insoluble particles (solids) from a liquid?

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Is the image above an image of an element, compound or mixture?

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Is the image above an image of an element, compound or mixture?

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Is the image above an image of an element, compound or mixture?

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What is the main difference between a compound and a mixture?

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What method of separation separates colours?

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Draggable itemCorresponding Item
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4.1.1.3 The Development of the model of the atom
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A chocolate chip cookie could be used as a model for JJ Thomson's theory of the structure of an atom.

Assess the model and write:

a) Two reasons it was a good model for JJ Thomson's theory
b) One reason why it is not a good model.

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Draw and label a diagram for

a) John Dalton's model
b) JJ Thomson's model

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Just like Rutherford, Jun is writing a conclusion from Geiger and Marsden's gold foil experiment. Help him write to explain the findings to show how the atomic model looked.

Jun needs to write:
a) The 3 different things that positive alpha particles did when fired at the gold foil
b) A conclusion for each of these findings
c) A description of the model of the atom that this new evidence provided

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Which of these belong to the Plum Pudding Model and the Nuclear Model?

  • Negative nucleus
  • Contains opposite charges
  • Made up of mostly empty space
  • No nucleus
  • Ball of negative charge
  • Ball of Positive charge
  • Contains protons
  • Contains only positive charges
  • Electrons moving
  • Contains electrons
  • Contains only negative charges
  • Electrons embedded - not moving
  • Positive nucleus
  • Plum Pudding
  • Nuclear Model
  • Both
  • Neither
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Draggable itemCorresponding Item
JJ Thomson
Bohr
Rutherford
Dalton
Chadwick
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Compare the nuclear model to the current model, giving both similarities and differences.

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Select two correct statements about Dalton’s model of atoms.

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Which is the best representation of Dalton's model?

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JJ Thomson said that there must be something smaller than an atom.

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True! He said there was something smaller - what are they called?

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Which image shows JJ Thomson’s model?

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JJ Thomson’s model was called the currant bun model.

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It was called the Plum Pudding model - why?

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What happened to the alpha particles in Rutherford's gold foil experiment?

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Which image shows Rutherford’s nuclear model?

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Which image shows Bohr’s model?

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What did later experiments show about the nucleus?

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What subatomic particle did James Chadwick suggest existed?

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Scientists noticed a difference in the atomic number and mass of an atom.

4.1.1.4 Relative electrical charges of subatomic particles
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What is the charge of a proton?

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What is the relative size of an electron?

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What is the charge of a proton?

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Why are atoms neutral? (hand mark)

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What is the charge of a proton?

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What is the relative size of an electron?

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What is the relative size of an electron?

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What is the charge of an ion formed when calcium loses 2 electrons?

4.1.1.5 Size and mass of atoms
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What is the atomic number of carbon?

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Which element has an atomic number of 11?

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How many protons does Hydrogen (H) have in its nucleus?

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What element in the periodic table has 8 protons?

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What is the proton number of Helium (He)?

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How many protons are in the nucleus of Carbon (C)?

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Correct the information so that Lucas can submit his homework:

The atomic number tells you how many __________ are in the nucleus of an atom. Each element has a unique __________ number. The atomic number is always the __________ of the two numbers found for each element on a periodic table. For an atom, the number of protons is __________ the number of electrons.
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How can the neutron number of an element be calculated?

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What is the neutron number of an Oxygen atom whose atomic number is 8 and mass number is 16?

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If an element has an atomic number of 6 and a mass number of 12, what is the number of neutrons?

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Li: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
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C: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
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Xe: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
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As Protons:_______ Electrons: _______
Neutrons: _______
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Be Protons:_______ Electrons: _______
Neutrons: _______
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In Protons:_______ Electrons: _______
Neutrons: _______
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Ne Protons:_______ Electrons: _______
Neutrons: _______
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Os Protons:_______ Electrons: _______
Neutrons: _______
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Zn Protons:_______ Electrons: _______
Neutrons: _______
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Sr Protons:_______ Electrons: _______
Neutrons: _______
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Au Protons:_______ Electrons: _______
Neutrons: _______
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Ta Protons:_______ Electrons: _______
Neutrons: _______
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Challenge: Atoms are very small, and their nucleus is even smaller. Research and explain the size of atoms and their nucleus.

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What are the protons, electrons and neutrons of Helium-3?
P: _______
E: _______
N: _______
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What are the protons, electrons and neutrons of Helium-4?
P: _______
E: _______
N: _______
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What are the protons, electrons and neutrons of Helium-6?
P: _______
E: _______
N: _______
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What are the protons, electrons and neutrons of Helium-7?
P: _______
E: _______
N: _______
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Find the symbol for helium on your Periodic Table.

Which of the isotopes has the mass number closest to the mass number given on the Periodic Table?

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Would the chemical properties of the isotopes of helium be the same or different?
Explain your answer. (hand mark)

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Give the symbol of the isotope described.

An isotope with 29 protons and 34 neutrons.

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Give the symbol of the isotope described.

An isotope with 13 protons and 13 neutrons.

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Give the symbol of the isotope described.

An isotope with 56 protons and 81 neutrons.

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Give the symbol of the isotope described.

An isotope with 3 protons and 6 neutrons.

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Give the symbol of the isotope described.

An isotope with 14 protons and 19 neutrons.

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What are the protons, electrons, and neutrons of the element Potassium? P: _______ E: _______ N: _______
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What element in the periodic table has 8 protons?

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This is Scandium.

What is its atomic number?

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How many protons does it have?

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What is its atomic mass?

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How many neutrons does it have?

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What is an isotope?

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They have a very _____ mass.

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Electrons are a ________ particle.

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They are located in ______ around the outside of an atom.

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Which element has an atomic number of 11?

4.1.1.6 Relative Atomic Mass
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Calculate the relative atomic mass (Ar) of gallium to 3sf given that it consists of two isotopes with these abundances: Ga-69 = 60.1%, Ga -71 = 39.9%.

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The data shows the mass numbers and abundances of naturally-occurring copper isotopes.

Cu-63 = 69%
Cu-65 = 31%

Calculate the relative atomic mass of copper. Give your answer to 1 decimal place.

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What is the relative atomic mass of element X with isotopes 20 (80%) and 22 (20%)?

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Calculate the relative atomic mass of isotope A (10, 50%) and isotope B (12, 50%).

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If 70% of isotope 35 and 30% of isotope 37, what is the relative atomic mass?

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Calculate the relative atomic mass of magnesium if Mg-24 has 78% abundance and Mg-26 has 22% abundance.

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Given Cl-35 at 75% and Cl-37 at 25%, find the relative atomic mass of chlorine.

4.1.1.7 Electronic Structure
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Match these elements to the correct electron configuration.

Draggable itemCorresponding Item
Carbon (C)
2,8
Sodium (Na)
2,8,1
Magnesium (Mg)
2,8,2
Fluorine
2,4
Neon (Ne)
2,7
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How many valence electrons does neon have?

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How many valence electrons does neon have?

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Match these elements to the correct electron configuration.

Draggable itemCorresponding Item
Fluorine
2,8
Sodium (Na)
2,8,1
Neon (Ne)
2,8,2
Carbon (C)
2,4
Magnesium (Mg)
2,7
Instructions: fill in the boxes below to show the electron configuration of these atoms. Use your periodic table to help you. The example above shows you how.
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Draw the electrons of Nitrogen

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Draw the electrons of Lithium

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Draw the electrons of Neon

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Draw the electrons of Magnesium

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Explain how electrons are arranged in electron shells

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Fluorine has 9 electrons. How are they arranged?

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Match the atom to its electron configuration

Draggable itemCorresponding Item
Potassium (19)
2,1
Lithium (3)
2,8,1
Sodium (11)
2,8,8,1
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Chlorine ion (Cl-) has fewer electrons than a chlorine atom (Cl).

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Atoms that lose electrons form positive ions.

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How many electrons does this have?

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What is the electron structure?

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How many electrons does this atom LOSE?

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How many electrons does this have?

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What is the electron structure?

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How many electrons does this atom LOSE?

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Draw the electron configuration for Sodium

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Draw the electronic structure of Chlorine

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Draw the electronic structure of Potassium

4.1.2.1 The Periodic Table
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4.1.2.2 Development of the Periodic Table
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Who is the creator of the Modern periodic table?

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What distinguished Mendeleev's Periodic Table?

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Why are elements in the same group in Mendeleev's periodic table?

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How did Mendeleev organise the elements in his periodic table?

4.1.2.3 Metals and non-metals
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Are most metals at room temperature solid, liquid, or gas?

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  • High density
  • Ductile (can be made into wires)
  • Lustrous (shiny)
  • Dull
  • Solid at room temperature
  • Gas or liquid at room temperature
  • Good conductor of electricity and Heat
  • Low density
  • Malleable (able to be hammered)
  • Poor conductor of electricity and heat
  • Brittle
  • Metal
  • Non-Metal
4.1.2.4 Group 0
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Describe the pattern of reactivity of these elements and others in their group

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4.1.2.5 Group 1
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List the names of the 6 elements that are known as the Alkali Metals

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For the first 3 elements draw the electron shell configurations

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How many electrons do they have on their outer shell?

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Draw the ion formed from the Li atom

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Draw the ion formed from the Na atom

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Draw the ion formed from the K atom

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Describe the pattern of reactivity of these elements.

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4.1.2.6 Group 7
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Draw the ion formed from the F atom

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Draw the ion formed from the Cl atom

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Describe the pattern of reactivity of these elements and others in their group

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4.1.3 Properties of Transition Metals
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Sort out the following elements whether they belong to Group 1 metals or Transition metals.

  • Copper
  • Iron
  • Sodium
  • Lithium
  • Transition Metal
  • Group 1 Metal
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Identify the property from the provided options:

  • Soft and can be cut with a knife
  • Dense
  • Low density
  • High melting point
  • React slowly with water
  • React vigorously with water
  • Produce alkaline solutions when react with water
  • Form coloured compounds
  • Group 1 Metals
  • Transition Metals
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Identify the property from the provided options:

  • Soft and can be cut with a knife
  • Dense
  • Low density
  • High melting point
  • React slowly with water
  • React vigorously with water
  • Produce alkaline solutions when react with water
  • Form coloured compounds
  • Group 1 Metals
  • Transition Metals