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Chemistry > Chemistry Test 7 > Flashcards

Chemistry Test 7 Flashcards

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1
Q

Draw the Lewis Dot diagram for Ammonia (NH₃)

A

. H
|
H —— N —– H
. .

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2
Q

Write the formula unit for Calcium (Ca) and Phosphorus (P)

A

Ca₃P₂

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3
Q

Draw the Lewis Dot diagram for PCl₃

A

.. .. ..
:Cl ——- P ——- Cl:
.. | ..
:Cl:
..

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4
Q

Write the formula unit for Potassium (K) and Nitrogen (N)

A

K₃N

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5
Q

What type of bond is I₂

A

covalent bond

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6
Q

What type of bond is Cu

A

Metallic Bond

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7
Q

What type of bond is Fe₃Al

A

Metallic Bond

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8
Q

What type of bond has attraction between oppositely charged ions?

A

Ionic Bond

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9
Q

What type of bond shares one or more electrons?

A

Covalent Bond

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10
Q

What type of bond does the electron-sea theory belong to?

A

Metallic Bonds

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11
Q

Covalent bonds create

A

Molecules

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12
Q

Ionic bonds create

A

Formula Units

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13
Q

Bonds between two nonmetals.

A

Covalent bonds

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14
Q

Bonds between a nonmental and a metal.

A

Ionic Bonds

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15
Q

Bonds between metals

A

Metallic Bonds

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16
Q

Diatomic molecules (naturally occurring.)

A

hydrogen (H2), nitrogen (N2), oxygen (O2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2)

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16
Q

(T or F) Diatomic elements such as I2 exhibit ionic bonding.

A

False

17
Q

(T or F) There are four unshared pairs of electrons in a water molecule.

A

False

18
Q

(T or F) The greater the difference in electronegativity between two elements, the greater the polarity of the resulting bond.

A

True

19
Q

Electrons are shared unevenly between two atoms due to a difference in their electronegativity.

A

Polar Compound

20
Q

A type of bond that occurs when two atoms share electrons equally.

A

A nonpolar compound

21
Q

(T or F) It is improper to refer to sodium chloride as a molecule

A

True

22
Q

(T or F) Ionic compounds have considerably lower boiling points than polar covalent compounds have.

A

False

23
Q

Chemical bonds between atoms involve the rearranging of __________ to maximize stability.

A

Electrons

24
Q

What type of bond would you expect in a compound of oxygen and sodium?

A

Ionic

25
Q

The electron-sea theory accounts for all the following characteristics of metals such as.

A

Luster, conductivity, and ductility

26
Q

An orderly arrangement of ions in a 3D pattern within a compound is called a(n) _________.

A

Crystal Lattice

27
Q

Why do atoms bond?

A

To gain stability and lose energy.

28
Q

A bond that forms between two or more atoms that have high electron affinities is most likely a(n) ____________.

A

Covalent Bond

29
Q

Examples of nonpolar covalent molecule.

A

F2, O2, Br2

30
Q

The polarity of a bond depends on the difference in the atom’s ____________.

A

Electronegativities

31
Q

To achieve the octet when combining with potassium, would an atom of a Group 16 element be expected to lose, gain, or share electrons?

A

Gain

32
Q

The attraction between opposite electrical charges; holds covalent bonds together.

A

Electrostatic Force

33
Q

Most metals are likely to freely share electrons when bonding with each other because they have ______________.

A

Low electronegativities

34
Q

What is associated with ionic compounds?

A

Opposite charges attracting each other, hard, brittle solids, and formula units.

35
Q

Compounds formed by the attraction between oppositely charged ions are the result of _______.

A

Ionic Bonds

36
Q

The electron shared in a covalent bond are called a(n) _____________.

A

Bonding Pair

37
Q

Although they are made of two or more atoms, _______ often act as single charged particles in chemical reactions and solutions.

A

Polyatomic ions

38
Q

A mixture of atoms of a metal with another element where the mixture has metallic properties is called a(n) _____________.

A

Alloy

39
Q

In general, how do the stability and energy of bonded atoms compare with that of unbonded atoms?

A

Stability is greater and energy is lower for bonded atoms.

40
Q

How do intermolecular forces affect the melting point of a compound?

A

Stronger intermolecular forces within a compound increase the melting point.

Chemistry (4 decks)

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