Brainscape's Knowledge GenomeTM

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


See full index

Chemical Bonds > Chemical Bonds Quiz 1 > Flashcards

Chemical Bonds Quiz 1 Flashcards

1
Q

when a new bond is formed, energy is (released/absorbed)

A

RELEASED - making it an exothermic process

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

when a bond is broken, energy is (released/absorbed)

A

ABSORBED- making it an endothermic process

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

IT TAKES ENERGY TO BREAK A BOND

A

!!!!

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

when does bonding occur?

A

when electrons are shared or transferred between atoms (all about valence electrons!!)

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

the number of valence electrons involved determines the bonding ratio

A

life hack: CRISS CROSS oxidation states with subscripts

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

Metallic Bonds

A

occur between metals

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

Ionic Bonds

A

transfer of electrons between metals and non metals

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

Covalent Bonds (x2)

A

sharing of electrons between nonmetals (two types: polar covalent and non polar covalent)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

_____atoms are surrounded by a sea of mobile electrons. this free electron behavior accounts for conductivity and magnetism.

A

METAL

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

why are metallic bonds possible?

A

because metals have very few valence electrons with low ionization energies.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

why are metals malleable?

A

because the atoms are free to move to new locations while the “sea” of electrons still surround them.

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

what does an IONIC BOND result from?

A

the attraction between two oppositely charged ions (metal and nm)
example: sodium and chlorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what are ionic compounds?

A

crystal lattices of positive and negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ALL COMPOUNDS WITH POLYATOMIC IONS HAVE BOTH COVALENT AND IONIC BONDING!!

A

!!!!

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

what are ANIONS?

A

(ionic bonds) negatively charged- non metals and most polyatomic ions

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

what are CATIONS?

A

(ionic bonds) positively charged - metals and few polyatomic ions

17
Q

why do ions bond to other ions?

A

SO THAT THE CHARGE IS NEUTRALIZED! also- each ion has a full octet of electrons

18
Q

characteristics of IONIC SOLIDS?

A
  • very strong force holding oppositely charged ions together
  • high melting point, high boiling point
  • can dissolve in water and dissociate (ions come apart)
  • the solution of ions can then conduct electricity (= electrolytes)
19
Q

molecular solids?

A
  • formed by covalent bonding (either polar or non polar)
  • form individual models which can attract to each other
  • easily melted and boiled
  • soft solids (wax, butter, ice)
20
Q

network solids?

A
  • typically formed by non polar covalent bonding
  • does NOT form separate molecules
  • forms one single crystal made of nonmetal atoms connected by one continuous network of covalent bonds with no areas of weakness that can break apart.
  • ex- quartz, diamonds, sapphires
  • do not conduct electricity, poor conductors of heat
  • hard but brittle
21
Q

in a single covalent bond ___ electrons are shared between two atoms

A

2

22
Q

atoms share _____ electrons to form a double bond

A

4

23
Q

atoms share ____ electrons to form a triple bond

A

6

24
Q

All ELECTRONS MUST BE PAIRED!!!

A

!!!

25
Q

Non Polar Covalent Bonds

A

electrons are shared equally and are just as likely to be found around either molecule

26
Q

Polar Covalent Bonds (H2O!!!)

A

electrons are shared UNEQUALLY and electrons are more likely to be around one atom (the more electronegative atom hogs the electrons!)

27
Q

POLARITY = ________

A

separation of positive and negative charge

28
Q

Non-Polar Bond=

A

bonding electrons are shared equally

29
Q

Polar Bond =

A

electrons are shared UNEQUALLY

30
Q

how do you determine if a bond is polar?

A

look at electronegativity difference (table s, subtract)

31
Q

all polar molecules contain polar covalent bonds but just because a molecule has polar covalent bonds doesnt mean it is a polar molecule.

A

!!!

32
Q

EN DIFFERENCE:

1.7 (large) = Ionic

A

!!!

33
Q

Polarity in BOND vs. Polarity in MOLECULE

A

Polar Covalent Bonds: occur when the bond is between two atoms with different electronegativities

Polar Molecules: must have polar covalent bonds and an asymetrical shape

34
Q

_____ are the forces that hold atoms together in compounds or molecules

A

chemical bonds

Chemical Bonds (1 decks)

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