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Questions and Answers
Questions and Answers
Which of the following best describes the arrangement of elements in the modern periodic table?
Which of the following best describes the arrangement of elements in the modern periodic table?
- Alphabetically by element name.
- By increasing atomic number. (correct)
- By similar reactivity.
- By increasing atomic mass.
What information can be directly gathered from the group number of a main group element?
What information can be directly gathered from the group number of a main group element?
- The atomic mass of the element.
- The total number of electron shells in an atom of the element.
- The number of electrons in the outermost shell of an atom of the element. (correct)
- The number of protons in the nucleus of an atom of the element.
How does reactivity change as you move down Group 1 (alkali metals) in the periodic table?
How does reactivity change as you move down Group 1 (alkali metals) in the periodic table?
- Reactivity decreases due to increasing ionization energy.
- Reactivity remains constant as elements in the same group have similar properties.
- There is no predictable pattern of reactivity within Group 1.
- Reactivity increases due to added electron shells and a weaker hold on outer electrons. (correct)
Which of the following properties is NOT generally associated with metals?
Which of the following properties is NOT generally associated with metals?
Which of the following describes the general trend in atomic size as you move across a period (from left to right) in the periodic table?
Which of the following describes the general trend in atomic size as you move across a period (from left to right) in the periodic table?
Which of the following is a characteristic property of noble gases?
Which of the following is a characteristic property of noble gases?
What type of bonding typically occurs between non-metal atoms?
What type of bonding typically occurs between non-metal atoms?
In ionic bonding, what is the usual process that occurs between metal and non-metal atoms?
In ionic bonding, what is the usual process that occurs between metal and non-metal atoms?
What is a common characteristic of transition elements?
What is a common characteristic of transition elements?
Compared to non-metals, which of the following is a characteristic property of metals related to their ability to conduct electricity?
Compared to non-metals, which of the following is a characteristic property of metals related to their ability to conduct electricity?
Which of the following best describes the properties of metalloids?
Which of the following best describes the properties of metalloids?
What is an alloy?
What is an alloy?
Which of the following best describes the force involved in metallic bonding?
Which of the following best describes the force involved in metallic bonding?
What happens to the melting point and changes in state as the atomic number increases within a group of non-metals?
What happens to the melting point and changes in state as the atomic number increases within a group of non-metals?
Which of the following are diatomic molecules?
Which of the following are diatomic molecules?
When metal atoms lose electrons, what type of ions do they form?
When metal atoms lose electrons, what type of ions do they form?
Consider element X, which reacts violently with water. In which group of the periodic table is element X most likely located?
Consider element X, which reacts violently with water. In which group of the periodic table is element X most likely located?
What is the valency?
What is the valency?
What is the difference between ductile and malleable properties of metals?
What is the difference between ductile and malleable properties of metals?
How did Mendeleev arrange the periodic table?
How did Mendeleev arrange the periodic table?
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Flashcards
Flashcards
Periodic Table
Periodic Table
Arranged by increasing atomic number. Vertical columns are Groups, horizontal rows are Periods.
Groups (Periodic Table)
Groups (Periodic Table)
Vertical columns of elements with similar properties in the periodic table.
Periods (Periodic Table)
Periods (Periodic Table)
Horizontal rows in the periodic table that arrange elements.
Alloy Definition
Alloy Definition
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Reactive Metals
Reactive Metals
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Transition Elements
Transition Elements
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Metalloids
Metalloids
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Non-Metals
Non-Metals
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Group Properties
Group Properties
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Periods
Periods
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Metals
Metals
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Malleable
Malleable
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Ductile
Ductile
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Sonorous
Sonorous
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Non-Metals
Non-Metals
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Noble Gases
Noble Gases
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Transition Elements
Transition Elements
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Chemical Bonding
Chemical Bonding
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Ions
Ions
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Non-metal + Non-metal compounds
Non-metal + Non-metal compounds
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Study Notes
Study Notes
- Chemistry C3 summary of key concepts.
Periodic Table
- In 1869, Mendeleev created the periodic table.
- Only 61 elements were known at the time, 32 of were included in the table.
- Elements are arranged in order of increasing atomic number.
- Vertical columns arrange elements with similar properties, known as Groups
- Groups indicate the quantity of electrons in each shell.
- Horizontal rows arrange the elements in Periods.
- Alloys are mixtures of elements designed for specific properties.
Groups
- Reactive Metals: Group I (alkali), Group II (alkali earth metals)
- Transition Elements
- Poor Metals
- Metalloids
- Non-Metals: Group VII - (halogens)
- Noble Gas
Electron Arrangement
- Elements in the same group have the same number of electrons on the last shell
- For the main group, the number represents the number of electrons in the outer shell
- Periods also have numbers, indication the number of shells the atoms has
Metals
- Metals conduct electricity and are malleable and ductile.
- Usually solids, except for mercury, which is a liquid at room temperature.
- Metals have a high melting/boiling point
- They are good conductors of electricity and heat.
- Malleable metals can be changed by hammering
- Ductile metals can be pulled out to create wires
- Metals create a ringing sound when struck and are known as sonorous.
Non-Metals
- Non-metals do not conduct electricity and are neither malleable nor ductile.
- Non-metals are usually solid or gases
- Bromine is an exception in that it exists as a liquid at room temperature
- They also have a low melting/boiling point
- Bad conductors of electricity and heat
- Non-metals are very soft and brittle when solid
- Are not sonorous, malleable or ductile
- Reactivity decreases down the group
- An increase of melting point and changes occur
- Goes from gas to solid as atomic number increases
- Poisonous and give off a strong similar smell
- Combines power of atoms or groups of one
- Forms compounds with similar formulas
- Produces a series of compounds with other elements: chlorides, bromides, and iodides → Halides
- Halogens can react directly with metals to form METAL HALIDES
- They all form NEGATIVE IONS carrying a single charge
Noble Gases
- Noble gases don't react or combine with each other to form molecules or other compounds.
- Noble gases have very low melting/boiling points
- Discovered late due to lack of reactivity
- They have a very stable electron arrangement and thus, have no need of a bond or reaction
- Higher the group, the atomic size decreases
- Lower the period, the atomic size decreasing
Transition Elements
- The most useful metallic elements available between group ii and group iii since they are transitioning.
- Transition elements are hard and strong
- They have high density
- High melting/boiling point
- Many compounds are colored (metal salts dissolve and give color)
- Often show more than one valency - form more than 1 type of ion
- Iron and copper are examples
Chemical Bonding
- Involves the outer shell of electrons of each atom
- Elements comprises more than one separated atom individually arranged. Oxygen (02) or Hydrogen (H2) are DIATOMIC MOLECULES
- Most elements forming structures are metals, held together by metallic bonding, resulting in metal lattices
- Non-metallic elements require covalent bonding or exist as separate atoms (noble gases), resulting in simple or giant molecule lattices
Ions
- A charged particle; atom that has lost or gained electrons.
- Metal atoms easily lose electrons than gain, becoming positive ions. Results in a more stable arrangement.
- Non-metal atoms gain electrons to become negative ions. Results in a stable electron arrangement, similar to the nearest noble gas in the periodic table.
Ionic Compounds
- When a compound of metal + non-metal generally adopts a third type of bonding.
- Transfer of electrons from one atom to another.
- Transferring electrons result in the formation of positive and negative ions.
- Oppositely charged ions are held together by forces of attraction.
Metallic Bonding
- Bonding for metals.
- Sea of electrons form when metal atoms are closely packed together, they lose electrons of last shell
- They become a not electrically neutral, it now a positive ion since the number of protons changed) → creates an electrostatic force that holds the structure together.
Covalent Bonding
- Formed by the sharing of elements.
- Each atom gains electrons
- Forces of attraction between the shared electrons and the nuclei are greater than any repulsive force and results in molecules held together by the covalent bond.
Ionic Bonding
- Transfer of electrons between atoms produces oppositely charged particles known as ions which result in a different type of chemical bonding.
- Result from the attraction between oppositely charged ions.
- Metal atoms always lose their outer electrons to form positive ions
- The number of positive charges on a metal ion is equal to number of electrons lost
- Non-metal ions (except hydrogen) always gain electrons to become negative ions
- Number of negative charges on non-metals ion is equal to number of electrons gained
- Non-metal + Non-metal compounds are held together by a covalent bonding, creating a compound
- Metal + Non-Metal compounds are held together by ionic bonding between positive and negative ions
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