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10th grade > Chem Ch 6 Test > Flashcards

Chem Ch 6 Test Flashcards

1
Q

Why do atoms form bonds with each other?

A

Lose energy
Gain stability

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2
Q

An atom becomes more stable by bonding with another atom if the resulting electron configuration is more like that of what group of elements?

A

Noble gases

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3
Q

When atoms form bonds with each other, what is being rearranged between the atoms so that stability can be achieved?

A

Valence electrons

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4
Q

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

A

Covalent

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5
Q

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

A

Ionic

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6
Q

What type of bond would you expect in a compound of Nitrogen and Potassium?

A

Ionic

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7
Q

The measure of an atom’s ability to attract electrons to itself in a chemical bond is called

A

Electronegativity

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8
Q

The polarity of a bond depends on the difference in the atoms’

A

Electronegativity

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9
Q

Which of the following is a nonpolar covalent compound?
a. KCl
b. H2
c. KO
d. Cu

A

B

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10
Q

Which of the following values for EN would represent a bond that is mostly ionic?
a. 0.5
b. 1.9
c. 2.2
d. 2.8

A

D

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11
Q

Diatomic molecules

A

BrINClHOF
Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine

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12
Q

What do we call the attraction between opposite electrical charges?

A

Electrostatic force

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13
Q

If the atoms below formed a covalent compound, which is most likely to be the central atom?
a. helium c. chlorine
b. carbon d. sulfur

A

B

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14
Q

A dash in a Lewis structure represents __________ electron(s).

A

2

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15
Q

An orderly arrangement of ions in a three-dimensional pattern within a compound is called a(n)

A

Crystal lattice

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16
Q

Alloy

A

Mixture of 2 or more metals
Carry electrical current and thermal energy
Have luster
Malleable
Ductile
Ex: Wedding rings

17
Q

What gives metal its luster electrical and heating conductive abilities?

A

The free electrons that freely move around

18
Q

List the 3 properties of ionic compounds

A

Strong bonds
High melting points
Dense, brittle, hard
Good electron conductors if dissolved/molten

19
Q

List the properties of covalent compounds

A

Low melting point (weak attractions between atoms)
Not dense/hard
Poor heat and electricity conductors

20
Q

Which of the following molecules would you say has a double bond in it?
CO CO2 H2 H2O NaCl

A

CO2

21
Q

The luster or shine seen on most metals is thought to be caused by the movement of

A

Electrons

22
Q

In order to achieve an octet when combining with potassium, an atom of a Group 16 (6A) element would be expected to __________ electrons.

A

Gain

23
Q

An orderly arrangement of ions in a three-dimensional pattern within a compound is called a(n)

A

Crystal lattice

24
Q

The electron-sea theory accounts for all of the following characteristics of metals except

A

Brittleness

25
Q

A mixture of atoms from multiple metals which has metallic properties is called a(n)

A

Alloy

26
Q

Second law of thermodynamics

A

Things tend to lose energy
Atoms naturally want low energy

27
Q

Octet rule

A

Occurs when an atom has its full valence shell of electrons
Atoms give up or take electrons to fill up atom’s valence shell
Atoms is at its maximum stability

28
Q

Nonpolar vs polar covalent

A

Nonpolar- Electrons are shared equally
Polar- Electrons are shared unequally

29
Q

Electronegativity

A

Ability of an atoms in a bond to attract shared electrons
Depending on deltaEN, bonds range from nonpolar to highly polar to ionic

30
Q

Electrostatic force

A

+ and - charges in atoms that attract or repel each other

31
Q

Lewis structure

A

Notation for covalent bonds
Dot notation
Sharing valence electrons

32
Q

Polyatomic ions

A

Group of atoms that total charge is + or -
Charge tells us how many electrons group loses or gains
Often act as a unit, stay together during reactions

33
Q

Ionic bonding

A

Formed from a metal and nonmetal
Large deltaEN
Nonmetal steals the metal’s valence electrons
+ and - ions attract

34
Q

Formula unit

A

Ratio of cations to anion

35
Q

Metallic bonding

A

Electron-sea theory
Delocalized electrons (electrons don’t stay in their lvls)
Requires arrangement of metals in crystal lattice

36
Q

Network covalent substances

A

Covalently bonded into a 3 dimensional network
Ex: Diamonds, silicon
Hard and brittle
High melting points
Glassy lusters
Unusual electrical properties

10th grade (71 decks)

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