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Questions and Answers
Identify the group on the periodic table that contains elements with 7 electrons in their outer shell.
Identify the group on the periodic table that contains elements with 7 electrons in their outer shell.
Group 7 (Halogens)
What is the valency of elements in Group 5?
What is the valency of elements in Group 5?
3
Name a property shared by all elements in Group 0 (Noble Gases).
Name a property shared by all elements in Group 0 (Noble Gases).
They are all gases at room temperature.
Explain why Alkali Metals are stored under oil.
Explain why Alkali Metals are stored under oil.
What is the general chemical reaction that occurs when an alkali metal reacts with water?
What is the general chemical reaction that occurs when an alkali metal reacts with water?
Briefly describe a physical property that distinguishes Halogens from Noble Gases.
Briefly describe a physical property that distinguishes Halogens from Noble Gases.
What is the main reason for the chemical inertness of Noble Gases?
What is the main reason for the chemical inertness of Noble Gases?
How does the reactivity of Alkali Metals compare to that of Alkaline Earth Metals?
How does the reactivity of Alkali Metals compare to that of Alkaline Earth Metals?
What is the main purpose of the periodic table?
What is the main purpose of the periodic table?
How are elements organized in periods and groups in the periodic table?
How are elements organized in periods and groups in the periodic table?
What does the term 'valency' refer to in terms of elements?
What does the term 'valency' refer to in terms of elements?
What is the significance of the 'octet rule' in atomic theory?
What is the significance of the 'octet rule' in atomic theory?
How do you determine the valency of an element using its group number?
How do you determine the valency of an element using its group number?
What happens to an atom when it loses an electron?
What happens to an atom when it loses an electron?
Describe how to calculate the relative atomic mass (Ar) of an element with two isotopes.
Describe how to calculate the relative atomic mass (Ar) of an element with two isotopes.
If a dipositive ion, M2+, has 25 electrons, what is its atomic number?
If a dipositive ion, M2+, has 25 electrons, what is its atomic number?
What are isotopes?
What are isotopes?
How many electrons does an aluminium ion, 27 3+, have?
How many electrons does an aluminium ion, 27 3+, have?
Explain why relative atomic masses are rarely whole numbers.
Explain why relative atomic masses are rarely whole numbers.
Define mass number.
Define mass number.
Calculate the relative atomic mass of gallium given 60.1% gallium–69 and 39.9% gallium–71.
Calculate the relative atomic mass of gallium given 60.1% gallium–69 and 39.9% gallium–71.
What is the atomic number and how is it defined?
What is the atomic number and how is it defined?
Define relative atomic mass.
Define relative atomic mass.
What is the unique property of mercury (Hg) at room temperature compared to other metals?
What is the unique property of mercury (Hg) at room temperature compared to other metals?
Define isotopes and provide an example.
Define isotopes and provide an example.
What defines a metal based on electron behavior?
What defines a metal based on electron behavior?
How is mass number calculated for an atom?
How is mass number calculated for an atom?
What are the three sub-atomic particles that make up an atom?
What are the three sub-atomic particles that make up an atom?
Explain why all atoms are neutral.
Explain why all atoms are neutral.
What information does the atomic number (Z) provide?
What information does the atomic number (Z) provide?
Define relative atomic mass number (Ar).
Define relative atomic mass number (Ar).
Flashcards
Element
Element
A substance that cannot be broken down into simpler substances by chemical means or produced by combining simpler substances.
Periods
Periods
Horizontal rows on the periodic table where elements have the same number of electron shells.
Groups
Groups
Vertical columns on the periodic table where elements have the same number of electrons in their outermost shell (valence shell).
Valency
Valency
The number of electrons in an atom's outermost shell, which determines how many chemical bonds an element can form.
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Octet rule
Octet rule
A rule that states that most atoms try to attain eight electrons in their outermost shell when they bond to achieve stability.
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Atom
Atom
The smallest unit of an element that can exist independently and retain the chemical properties of that element.
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Proton
Proton
A positively charged particle found in the nucleus of an atom.
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Neutron
Neutron
A neutrally charged particle found in the nucleus of an atom.
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Electron
Electron
A negatively charged particle that orbits the nucleus of an atom.
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Nucleus
Nucleus
The central part of an atom where protons and neutrons reside.
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Atomic number
Atomic number
The number of protons in an atom's nucleus.
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Relative atomic mass number (Ar)
Relative atomic mass number (Ar)
The average mass of all known isotopes of an element.
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Isotopes
Isotopes
Atoms of the same element with the same number of protons but different number of neutrons.
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Alkali Metals
Alkali Metals
Elements with one electron in their outermost shell, making them highly reactive, soft metals with low densities. They tarnish quickly in air and react vigorously with water.
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Alkaline Earth Metals
Alkaline Earth Metals
Elements with two electrons in their outermost shell, making them reactive, slightly less reactive than alkali metals. The most common example is Magnesium, which reacts slowly with water.
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Halogens
Halogens
Elements with seven electrons in their outermost shell, making them highly reactive non-metals. They have low melting and boiling points and exist in different states of matter at room temperature: Fluorine and Chlorine are gases, Bromine is a liquid, and Iodine is a solid.
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Noble Gases
Noble Gases
Elements with eight electrons in their outermost shell (except Helium, which has 2), making them extremely unreactive. They are gases at room temperature and their boiling points increase as you move down the group.
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Mass Number
Mass Number
A measure of the total number of protons and neutrons in an atom's nucleus. This number can vary within an element, leading to isotopes.
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Relative Atomic Mass (Ar)
Relative Atomic Mass (Ar)
The average atomic mass of an element, taking into account the relative abundance of its isotopes.
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Relative Molecular Mass (Mr)
Relative Molecular Mass (Mr)
The average mass of a molecule of a compound compared to 1/12 the mass of the carbon-12 isotope, taking relative abundances of the naturally occurring isotopes into account.
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Metal
Metal
Any element that forms a positive ion (cation) by losing electrons.
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Diatomic Nonmetal
Diatomic Nonmetal
A non-metal that exists as a diatomic molecule at room temperature.
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Cation
Cation
A positive ion formed when an atom loses one or more electrons.
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Anion
Anion
A negative ion formed when an atom gains one or more electrons.
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Oxidation
Oxidation
A chemical reaction that involves the loss of electrons from an atom.
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Reduction
Reduction
A chemical reaction that involves the gain of electrons by an atom.
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What is atomic number?
What is atomic number?
The number of protons in the nucleus of an atom, which determines the element's identity.
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What is relative atomic mass (Ar)?
What is relative atomic mass (Ar)?
The weighted average of the masses of all the isotopes of an element, relative to the mass of carbon-12.
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What are isotopes?
What are isotopes?
Atoms of the same element that have the same number of protons but a different number of neutrons. They have the same atomic number but different mass numbers.
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What is the principle of the mass spectrometer?
What is the principle of the mass spectrometer?
A technique that separates ions based on their mass-to-charge ratio. It allows us to identify and measure the abundance of different isotopes.
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What is relative atomic mass (Ar)?
What is relative atomic mass (Ar)?
A measure of the average mass of an element's atoms, taking into account the relative abundance of its isotopes.
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How to calculate relative atomic mass (Ar)?
How to calculate relative atomic mass (Ar)?
The average mass of an atom of an element, calculated based on the masses and relative abundances of its isotopes.
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What is a molecule?
What is a molecule?
A group of atoms held together by chemical bonds.
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What is an ion?
What is an ion?
An ion is an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
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Atomic Theory
- Atomic structure consists of protons, neutrons and electrons
- Protons and neutrons are located in the atom's nucleus
- Electrons orbit the nucleus
- Atoms are neutral because the number of protons equals the number of electrons
- The number of protons defines the element
- Atomic number identifies the element
- Isotopes have same number of protons but different number of neutrons
- Mass number is the sum of protons and neutrons
- Relative atomic mass (Ar) is the average mass of all isotopes, taking into account their natural abundance
- Relative molecular mass (Mr) is the sum of the Ar values of all atoms in a molecule
- Elements are arranged in the periodic table by increasing atomic number
- Elements in the same group have similar chemical properties due to the same number of valence electrons
- Elements in the same period have same number of electron shells
- Metals tend to lose electrons to form positive ions(cations)
- Non-metals tend to gain electrons to form negative ions(anions)
- The periodic table shows trends in the physical and chemical properties of elements
Equations
- Metal + Oxygen → Metal Oxide
- Metal + Water → Metal Hydroxide + Hydrogen
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