Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 100 > Section 4 > Flashcards

Section 4 Flashcards

1
Q

What is the Minimum Energy Principle?

A

Atoms will react with each other so as to minimize their potential energy level.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is INTRAmolecular Bonding?

A

Bonds between atoms within the molecule (called chemical bonding)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is INTERmoleculucar Bonding?

A

Bonds between molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What do atoms do in relation to the minimum energy principle?

A

Atoms will bond with each other to obtain a lower potential energy level, which is the same thing as atoms becoming more stable.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Which group of atoms is the most stable?

A

The noble gases are very stable in their natural form, which also means they have a very low potential energy level.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why are noble gases so stable?

A

Noble gases are so stable due to the large potential energy gap between the valence shells. (between s & p)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What does it mean for atoms when a valence shell is full?

A

When a valence shell is full, the atoms are stable, the atom’s electrons are in a low potential energy well and become non-reactive.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are the 4 main characteristics of a noble gas?

A
  • They do not react
  • They must have the most stable electron configuration of the atoms
  • Their electron configurations a;; have full electron valence shells
  • The noble gas electron configuration must have the lowest possible energy level.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How do atoms react when they achieve the noble gas electron configuration?

A

All atoms become more stable and less reactive when they’ve achieved noble gas configuration.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the 4 key characteristics of chemical reactions?

A
  • Chemical reactions are the forming and breaking of chemical bonds
  • Reactions occur so atoms can go from a higher potential energy level to a lower potential energy level.
  • Atoms at their lowest potential energy level will not react readily
  • these un-reactive atoms are very stable.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the octet rule?

A

The octet rule is described as- the atoms will always to try fill their valence shell. All atoms will try to fulfill the octet rule to become more stable.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are the 4 key characteristics of the octet rule?

A
  1. Atoms with unfilled electron shells will react to fill their shells to become more stable.
  2. Hydrogen can lose one electron, or it can gain one electron to become more stable.
  3. All other atoms in the first pd will lose one electron to obtain a full valence shell.
  4. Atoms in the second and higher periods will react to obtain eight valence electrons as follows:
    - Atoms with 3 or less in their valence shell will lose electrons.
    - Atoms with 5 or more electrons in their valence shell will gain electrons.
    - Atoms with 4 electrons can either gain or lose 4 valence electrons.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are the different types of chemical bonds?

A
  • Ionic
  • Covalent
  • Metallic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is an Ionic chemical bond?

A

~Metal to non-metal,

~transfer of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is a Covalent chemical bond?

A

~non-metal to non-metal

~sharing of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is a Metallic chemical bond?

A

~metal to metal

~Giving off electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Atoms with 3 or less electrons in their valence shells will do what?

A

Atoms with 3 or less electrons in their valence shell will lose electrons to form cations, positively charged ions

18
Q

Atoms with 5 or more electrons in their valence shells will do what?

A

Atoms with 5 or more electrons in their valence shell will gain electrons to form anions, negatively charged ions.

19
Q

What is the charge on atoms with extra electrons?

A

Atoms with extra electrons are negatively charged.

20
Q

What is the charge on atoms with a deficiency of electrons?

A

Atoms with a deficiency of electrons are positively charged.

21
Q

What is the charge for the Alkali metals (Group IA)?

A

Alkali metals have a +1 charge

22
Q

What is the charge for Alkaline earth metals (Group IIA) ?

A

Alkaline earth metals have a +2 charge.

23
Q

What charge will Group IIIA have?

A

Group IIIA will have a +3 charge.

24
Q

What charge will Group VA have?

A

Group VA will have a -3 charge.

25
Q

What charge will Group VIA have?

A

Group VIA will have a -2 charge.

26
Q

What charge will Halogens (Group VIIA) have?

A

Halogens will have a -1 charge.

27
Q

What is the definition of an ionic compound?

A

An ionic compound is a compound composed of metal atoms bonded to a non-metal atom.

28
Q

What causes an ionic bond?

A

An ionic bond is caused by the attraction of the positive cation to the negative anion. The bond is an electrostatic attraction of the ions.

29
Q

What is a polyatomic ion?

A

There are many polyatomic ions. These are ions that have two or more atoms covalently bonded together.

30
Q

What produces crystal lattice forms?

A

The positive and negative charges associated with the ions cause the ions to be attracted to each other, forming crystal lattice.

31
Q

Is an ionic compound’s melting point high or low?

A

An ionic compound’s melting point is high.

32
Q

T or F: Ionic compounds are soluble in water.

A

TRUE

33
Q

What do solutions made from ionic compounds conduct?

A

Solutions made from ionic compounds conduct electricity.

34
Q

What is electronegativity?

A

In covalently bonded molecules, some atoms have a larger attraction toward the electrons then others. This tendency to attract electrons is measured by electronegativity.

35
Q

Which way on the periodic table do you have to move for electronegativity to increase?

A

As you go across the table from left to right or go up, the atom;s electronegativity increases.

36
Q

How can you tell if something is non-polar?

A

When two atoms come together and form a covalent bond and their difference in their electronegativity is 0.5 or smaller.

37
Q

How can you tell if something is polar?

A

When two atoms come together to form a covalent bond and the difference in their electronegativity is between 0.5 and 1.5. (Polar covalent)

38
Q

How are dipoles created?

A

Covalently bonded molecules with polar covalent bonds create dipoles.

39
Q

What is the relationship between the difference in electronegatives and dipoles?

A

The larger the difference in the electronegatives, the greater the dipole.

40
Q

What does the difference in electronegativity have to be for the bond to be ionic?

A

The difference in electronegativity is greater than 2.0, the bond is ionic.

41
Q

What are the degrees for the 3 geometric shapes?

A

Linear: 180.
Trigonal: 120.
Tetrahedral: 109.

42
Q

How do you determine the net molecular polarity?

A

By combining the geometry of the molecule and the dipole associated with each bond.

Chem 100 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions