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Chemistry 6 > Quest > Flashcards

Quest Flashcards

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1
Q

Pseudo-noble

A 
Pseudo-noble has electron configuration 
• elements to the right of silver also form pseudo-noble gas configurations when forming an ion 
• Gold 
• Copper
• Cadmium
• Mercury
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2
Q

Formation of anions

•

A

an anion is produced when an atom gains one or more valence electrons
• The name fo an anion of a nonmetallic element is NOT the same as the element name
• The name of the element partially ends in -ide
• Chlorine/Chloride oxygen/oxide
• atoms of nonmetallic elements attain noble-gas electrons more easily by gaining electrons than by losing them because these atoms have relatively full valence shells
• Cl 1s^22s^22p^63s^23p^5. Cl^- 1s^22s^22p^63s^23p^6
• the chloride ion has a single negative charge
• Note that the electron configuration of chloride is the same of that of an argon atom
• Chlorine atoms, need one more valence electron to achieve the electron configuration of the nearest noble gas

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3
Q

Halide ions

A

ions produced when atoms of chlorine and other halogens gain electrons
• All halogens have 7 valence electrons and need only one electron to achieve the noble gas configuration

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4
Q

Formation of Ionic compounds

A
  • an Ionic compound is a compound composed of cations and anions
  • Although they are composed of ions and Ionic compounds are electrically neutral
  • The total negative charge of the cations equals the total negative charge of the anions
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5
Q

Ionic bonds

A

the electrostatic forces that hold ions together in Ionic compounds are called Ionic bonds

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6
Q

Chemical formula

A

a chemical formula shows the number of atoms of each element in the smallest representative unit of a substance
• Sodium chloride = NaCl
• NaCl does not represent a single physical unit

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7
Q

Formation of sodium chloride

A

sodium cations and chloride anions form a repeating 3-dimensional array in sodium chloride (NaCl)

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8
Q

Formula unit

A

Ionic compounds do not exist as a single discrete unit, but as a collection of positively and negatively charged ions arranged in repeating patterns
• The chemical formula of an Ionic compound refers to a ratio known as a formula unit
• It is the lowest whole-number ratio of ions in an Ionic compound

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9
Q

Properties of Ionic compounds

A

most Ionic compounds are crystalline solids at room temperature
• The component ions are arranged in 3-dimensional patterns
• There is a large attraction force since each sodium ion is surrounded by 6 chlorine II s and 6 chlorine ions are surrounded by 6 sodium atoms
• Ionic compounds generally have high melting points
• Because of the arrangement of 6 ions surrounded by 6 ions there is a very strong attraction force and minimal repulsion
• This results in very stable structure
• This stability is reflected in the fact that NaCl has a melting point of about 800 celcius
• Ionic compounds can conduct an electric current when melted or dissolved in water
• The orderly structure breaks down
• If a voltage is applied across this molten mass, cations migrate freely to one electrode and anions migrate to the other
• This allows electric current to flow between the electrodes through an external wire

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10
Q

Coordination number

A

Coordination Number
• the coordination number is the number of ions of opposite charge that surround the ion in a crystal
• Sodium is surrounded by 6 chloride ions and chloride ions are surrounded by 6 sodium ions therefore the coordination number for sodium and chloride is 6

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11
Q

Metallic Bonds and Metallic Properties

A
  • the valence electrons of atoms in a pure metal can. E modeled as a sea of electrons
  • This means that the electrons are mobile and can drift freely from one part of the metal to another
  • Metallic bonds are the forces of attraction between the free-floating valence electrons and the positively charged metal ions
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12
Q

Properties of metal

A
  • conductivity
  • Ductile
  • Malleable
  • Low volatility
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13
Q

Crystalline structure of metals

A

• metals are crystalline
• Metal atoms are arranged in very compact and orderly patterns
• For spheres of identical side, such as metal atoms, several closely packed arrangements are possible
1. Body centered cubic
2. Face centered cubic
3. Hexagonal close-packed

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14
Q

Body centered arrangement

A 
• every atom has 8 neighbors 
• Metallic elements: 
 - chromium 
 - sodium 
 - potassium 
 - iron 
 - tungsten
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15
Q

Face Centered arrangement

A 
• every atom has 12 neighbors 
• Examples
 - gold 
 - copper
 - silver 
 - aluminum 
 - lead
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16
Q

Hexagonal close-packed crystal structure

A

• examples:

  • zinc
  • magnesium
  • calcium
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17
Q

Alloys

A
  • a mixture of two or more elements at least one of which’s a metal
  • Copper + zinc = brass
  • Copper + tin = bronze
  • Steel
  • Alloys are important because their properties are often superior to those of their component elements
18
Q

Substitutional Alloy

A

• if the atomic sizes are similar the atoms can replace each other

19
Q

Interstitial Alloy

A
  • if the atomic sizes are quite different, the smaller atoms can fit into the spaces between the larger atoms
  • For steel. Carbon toms occupy the spaces between the iron atoms
20
Q

• elements within each group of the periodic table react in a similar way because they have the same number of _________ _________

A

Valence electrons

21
Q

• Valence electrons are the electrons in the __________ occupied energy level of an elements atoms

A

Highest

22
Q

• These valence electrons determine the

A

the chemical properties of an element.

23
Q

• To find the number of valence electrons in an atom of a representative element simply look at its
•

A

Group number

24
Q
  • Exceptions to the rule
  • atoms of helium have how many valence electrons
  • All of the other noble gases have how many valence electrons
A
  • 2

- 8

25
Q

Electron Dot Structures

A
  • valence electrons are the only electrons involved in chemical bonds
  • The valence electrons are shown in electron dot structure
26
Q

Lewis dot structure

A

• all noble gases have eight dots because their outer shell is completely full

27
Q

The Octet rule

• noble gases are ________ or ________ in chemical reactions

A

stable or non reactive

28
Q
  • The octet rule states that in forming compounds, atoms tend to achieve the electron configuration of noble gases
  • An octet is a set of
  • Noble gases have _______ electrons in their highest occupied energy level except for ______
  • Atoms of metals tend to ____ atoms, leaving a complete octet in the next lowest energy level
  • Atoms of some nonmetals tend to _____ electrons or to share electrons with another nonmetal atom or atoms to achieve a complete octet.
A
  • atoms tend to achieve the electron configuration of noble gases
  • eight
  • eight electrons, helium
  • lose
  • gain
29
Q

Formation of cations
• an atom is electrically ______ because it has the same number of _____ and ________
• An ion forms when an atom ______or ______electrons
• A positively charged ion or a cation is produced when an atom _____ one or more valence electrons

A
  • neutral, protons and electrons
  • loses or gains
  • loses
30
Q

Cation
• for metals the name of the cations is the same as the
• Sodium atom forms a sodium cation (Na^+)
• Calcium atoms forms a calcium cation (Ca^2+)
• although their names do not change, it is highly possible that cations have big chemical differences when compared to the metal
• Sodium reacts explosively with water
• Sodium cations are quite non reactive (part of table salt)

A
  • name of the element
31
Q

Group 1A cations

  • the most common cations are those produced by the _____ of valence electrons from metal atoms
  • Sodium can lose an electron to become a positively charged sodium ion.
  • A sodium ion has an electrical configuration similar to the noble gas neon
A
  • loss
  • Sodium can lose an electron to become a positively charged sodium ion.
  • A sodium ion has an electrical configuration similar to the noble gas neon
32
Q

Representing cations

• you can represent the loss of an electron or ionization of the sodium atom by writing the complete

A

electron configuration of the atom and the ion formed

33
Q

Group 2a cations
• magnesium atom attains the electron configuration of a neon atom by losing two valence electrons and producing a magnesium cation with a charge of 2+
• The atoms of metals lose the number of electrons necessary to attain the electron configuration of a ________ _____
• 1A metals lose one electron
• 2a metals lose two electrons

A

Noble gas

34
Q

Transition metal cations

A

Transition metal cations
• the charges of cation of the transition metals may vary
• Iron can lose two electrons forming Fe^2+
• Iron can also lose three electrons forming Fe^3+
• Some ions for we by transition metals do not have noble gas electron configurations (ns^2np^6) and are therefore are exceptions to the octet rule

35
Q
  • ions with charges of 3 or greater are uncommon
  • Silver does not attain a noble gas configuration
  • If silver loses its 5s^1 electron forming a positive ion Ag+ the configuration results in the 4s^24p^6
  • With electrons in the highest occupied energy level and all of the orbitals filled is favorable
  • This is a pseudo-noble gas configuration
A

Ok

36
Q

How do chemists model the valence electrons of metal atoms

A

Chemists can Model the valence electrons of metal atoms into body centered cubic, face centered cubic, and hexagonal close-packed

37
Q

Why are alloys more useful than pure metals

A

Alloys are more useful than our metals because their properties are often superior to those of their component elements

38
Q

Define ductile and malleable

A

Ductile means that if you pull it then it will stretch before it breaks
Malleable means that you can hit really hard with something and it will only bend

39
Q

Why is it possible to bend metals but not Ionic crystals

A

It is possible to bend metals because they have a sea of flowing electrons that can move around but Ionic crystals don’t have that so you can not bend ionic crystals

40
Q

Name two widely used alloys and describe their uses

A

Copper + tin = bronze and steel are both widely used alloys. They can be found in tools, buildings, and many other things

Chemistry 6 (8 decks)

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