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Chemistry > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

What is the most important factor affecting how atoms form chemical bonds?

A

The number of valence electrons in each atom involved.

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2
Q

What is an attractive force between atoms that is strong enough to enable the group to act as a unit?

A

A chemical bond

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3
Q

What is the octet rule?

A

The statement that the valence shell of an atom wants to have eight electrons.

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4
Q

Elements toward the left of the periodic table tend to ________ electrons in bonding, while elements toward the right of the periodic table tend to _________ electrons in bonding.

A

Lose

Gain

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5
Q

What is a chemical bond in which positively charged ions are electrically attracted to negatively charged ions?

A

Ionic bond

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6
Q

The elements on the ______ of the periodic table- metals -react with those elements on the far ______- nonmetals (excluding the noble gases) -to form ionic crystalline solids.

A

Left side

Far right

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7
Q

What should we associate covalent bonding with?

A

Sharing electrons

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8
Q

What is a chemical bond that results from the sharing of valence electrons between atoms?

A

A Covalent bond
The mutual attraction of both positive nuclei for the negatively charged electron cloud holds the nuclei together in a covalent bond.
Each paired electron results in a single covalent bond.

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9
Q

When two atoms share a single pair of electrons, the bond is what?

A

a Single Bond

A single covalent bond

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10
Q

When atoms share two pairs of electrons it forms a what?

A

Double bond

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11
Q

What is formed when atoms share three pairs of electrons?

A

A triple bond

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12
Q

Some substances containing covalent do not exist as discrete molecules, nor do they have the usual properties of covalent compounds, such as low melting points. These substances are known as ___________ because they are composed of billions or trillions of atoms that are bonded together into a single unit by strong covalent bonds.

A

Covalent network

Generally, covalent bonds hold atoms together in discrete molecules.

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13
Q

When two atoms share a single pair of electrons, the bond is what?

A

a Single Bond

A single covalent bond

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14
Q

When atoms share two pairs of electrons it forms a what?

A

Double bond

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15
Q

What is formed when atoms share three pairs of electrons?

A

A triple bond

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16
Q

Some substances containing covalent do not exist as discrete molecules, nor do they have the usual properties of covalent compounds, such as low melting points. These substances are known as ___________ because they are composed of billions or trillions of atoms that are bonded together into a single unit by strong covalent bonds.

A

Covalent network

Generally, covalent bonds hold atoms together in discrete molecules.

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17
Q

The chemical bonds that bind atoms together in a metal are what? Like in covalent bonds, these bonds involve in sharing, rather than the transfer of electrons.

A

Metallic bonds

The large number of freely circulating electrons gives metals their characteristic properties.

18
Q

In most cases, the what in compounds is not completely ionic, covalent, or metallic?

A

Bonding

19
Q

A bond is considered predominantly ionic if the electronegativity difference between the two bonded atoms is greater than what number?

A

1.7

20
Q

A covalent bond in which both atoms share electrons equally is what?

A

A Nonpolar bond

21
Q

A covalent bond in which electrons are shared unequally between atoms is what?

A

A Polar bond

22
Q

What is only a fraction of a full charge? What are they represented by?

A

Partial charge

Represented by the lower case Delta

23
Q

What is a bond or molecule that has a negative end and a positive end? It has two poles.

A

Dipole

24
Q

What term refers to a situation in which electrons are shared by more than two atoms?

A

Delocalization

25
Q

What are de localized atoms?

A

Atoms that circulate freely instead of being bound.

26
Q

What is a bonding situation called in which electrons are shared by more than two atoms?

A

Delocalization

27
Q

What theory uses an assumption to predict the shapes of molecules?

A

Valence-shell electron-pair repulsion

28
Q

What shape has four bonding pairs around the atom, 0 nonbonding pairs, the bond angles are 109.5 degrees apart, and are nonpolar or polar?

A

Tetrahedral

29
Q

What shape has three bonding pairs and 1 nonbonding pair, polar, and it’s bond angles are 107 degrees apart?

A

Trigonal pyramidal. Only the positions of atoms describe the molecule’s shape. Nonbonding electron pairs repel more than bonding pairs.

30
Q

What shape has 2 bonding pairs and 2 lone pairs, polar, and it’s bond angles are 105 degrees apart?

A

Angular

31
Q

What shape has 1 or 2 bonding pairs and 0 nonbonding pairs, nonpolar or polar, and it’s bonding angles are 180 degrees apart?

A

Linear

32
Q

What shape has 3 bonding pairs and 0 nonbonding pairs, nonpolar or polar, and it’s bond angles are 120 degrees apart?

A

Trigonal planar

33
Q

Whenever electrons in a covalent bond are shared unequally, the bond will be ______.

A

Polar

34
Q

Determining whether or not a molecule is a _________ __________ is important for deciding what forces of attraction exist between molecules- forces that affect many properties of substances.

A

Polar molecule. A molecule that has a symmetrical distribution of polar bonds will have no net dipole and will be nonpolar.

35
Q

Many properties of a substance result from forces between molecules called what?

A

Intermolecular forces

36
Q

What type of close-packed unit cells do most metals assume?

A

Close-packed metals normally assume the hexagonal close-packing shape.

37
Q

In what way does a liquid crystal have characteristics of both liquids and solids?

A

It can move freely and it can freeze.

38
Q

What are solids that have no ordered arrangement or pattern for the particles that compose them?

A

Amorphous solids

39
Q

What solid is characterized by particles arranged in a regular and repeating three-dimensional pattern?

A

Crystalline solids

40
Q

What is the simplest repeating unit in a crystalline solid?

A

Unit cell

41
Q

What are some unit-cell arrangements?

A

Simple cubic, body-centred cubic, and face-centred cubic

42
Q

What is one of the most efficient crystal structures?

A

Hexagonal close packing

Chemistry (5 decks)

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