Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Unit 1 Test > Flashcards

Unit 1 Test Flashcards

Matter and bonding

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Atomic number tells us what?

A

of protons and electrons ( only if atom is electrically neutral)

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

How to find # of neutrons

A

Atomic mass - protons

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

isotopes

A

an element with the same about of protons but differing neutrons

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

Isotopic abundance

A

the percentage of each isotope that exists in nature

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

RadioIsotope

A

radio active isotope with a unstable nucleus that breaks down

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

How is isotopic abundance relative to atomic mass

A

Atomic mass is the average mass of all isotopes x their isotopic abundance

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

What is an atom

A

Empty space with a central nucleus and an electron cloud

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

What is the nucleus made up of

A

Protons and neutrons

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

Atomic mass = what?

A

The mass of all the neutrons and protons ( electrons basicly weigh nothing)

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

What is paleoclimatology

A

The study of ancient climate change using isotopic abundance

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

periodic table

A

alkali metals
alkali earth metals
transition metals
non metals
metaloids
inner transition metals
halogens
noble gases
actinods
lanthernoids
representive metals ( everything but transiiton metals)

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

Cations

A

Metals that lose electrons to become positive charged ions

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

Anions

A

Non metals that gain electrons to become negativity charged ions

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

Periodic law

A

elements arranged in order of increasing atomic
elements with similar
chemical properties appear periodically

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

Chemical Reactivity

A

similar # of valance electron = similar chemical properties

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

Atomic Radius

A

length from center of nucleus to outermost electron

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

What happens to the atomic radius when you go down a group

A

Atomic radius increases because there are more shells = more shielding electrons which block the attraction between the nucleus and the outer most electron, electrons repel spreading out

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what happens to atomic radius when you move across periods

A

when you go left to right across and period the atomic radius decreases because there are more protons without an additional electron shell = higher effective nuclear charge ( attraction) to pull in the electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Cations become smaller why?

A

lost of an electron which increases effective nuclear charge ( more attraction between nucleus and electron bring the electrons closer) which makes the atom smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Anion become bigger Why?

A

Gain of electrons decreases effective nuclear charge causing the electrons to repel and spread out ( atom gets bigger)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Ionization Energy

A

the energy required to remove the outer most electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what happens to the ionization energy when the atom is smaller

A

it increases because the attraction to the nucleus is greater ( effective nuclear charge) needed more energy to remove the outer electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what happens to the ionization energy when the atom is big

A

it decreases because the attraction between the electrons and the nucleus is lower due to shielding electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why are atomic radius and ionization energy trends the opposite?

A

When atomic radius decreases ionization energy increases
when atomic radius decreases ionization increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

successive ionization energies

A

when trying to remove a core electron the ionization energy is very high because the electrons are held closer to the nucleus due to the effective nuclear charge is very high

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

electronegativity

A

tendency for a bonded atom to attract electrons
decreases going down groups increases moving left to right in periods

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

why do smaller atoms have high electronegativity

A

smaller atoms have a greater effective nuclear charge causing the electrons to be closer to the nucleus so the smaller atom will hold the shared election closer to its self then the larger bonded atom

28
Q

when do the protons stay in the nucleus

A

the protons are attracted to the neutrons

29
Q

what is nuclear force

A

the attraction between the protons and neutrons that is holding the nucleus together

30
Q

what is ionic radius

A

the distance from the outermost electron to the nulcues of an ion

31
Q

what are ions

A

atoms that have gained of lost electrons which now have a positive or negative charge

32
Q

what are sheilding electrons

A

an extra shell of electrons that block the attraction between the outermost electron and the nucleus

33
Q

lewis dot diagrams

A

symbol= nucleus and core electrons
draw valance electrons
unpaired electrons= bonding electrons
paired electrons= lone pairs

34
Q

ionic bonding

A

metal and non metal
transfer of electrons
electrostatic attraction between ions
solid at SATP
form crystal lattice
END> 1.7

35
Q

why do ionic compounds exist as solids at room temperature

A

the electrostaic attarction between the cations and the anions is very strong = atoms are held very close together

36
Q

why do ionic compounds dissovle is water

A

the cations and anions of ionic compounds are attraction to the postive and negative dipoles of the water molecules surounding the ions breaking the ionic bonds

37
Q

why do ionic compounds have a high melting point

A

ioninc compounds have high melting points do to their strong electrostatic forces holding them together, a greater amount of energy is need to break the crystal lattice and overcome the ionic bonds

38
Q

why do ionic compounds conduct electrcity

A

when dissolved in water ionic compounds separate into cation and anions that move around bringing charge through the water

39
Q

why can you crush ionic compounds

A

ionic compounds form brittle ridge crystal lattices that when pressure is aplied crush into smaller piecies

40
Q

molecular compound

A

covalent bonds
intermolecular forces
electronegativites to close to transfers electrons
share electrons
two non metals
form single unit molecules

41
Q

pure covalent bond

A

END < 0.4
equal sharing of electrons

42
Q

polar covalent bond

A

0.4> END < 1.7
unequal sharing of electrons
partial charges

43
Q

cooridnate covalent bond

A

when one atom provides both electrons for a shared pair

44
Q

why do molecular compounds have low melting points

A

intermolecular forces are weaker than ionic bonds less energy is need to overcome the attraction

45
Q

do molecular compounds dissolve in water

A

pure covalent molecules do not dissolve in water do to the lack of oppsite charges to be attracted to the dipoles of water molecules

polar covalent molecules can dissolve in water due to their partial charged dipoles that attacted to the the dipoles of water molecules

46
Q

what is a polar molecule

A

partially negative and positive ends (poles)
can have polar bonds but not be a polar molecule
asymmetrical

47
Q

do molecular compounds conduct electricity

A

pure covalent molecules do not conduct electricity lack of oppsitie charges to charge the water

polar molecules are partial conductors do to partial charges that bring charge through the water

48
Q

molecular compound hardness

A

intermolecular forces are weaker than ionic bonds and do not form crystal lattices this causes molecular compounds to be more flexible and compressable

49
Q

what are intramolecular forces

A

the forces of attraction within a molecules or compound
( chemical bonds)
ionic bond
covalent bond
poalr covalent
cooridnate covalent

50
Q

what are intermolecular forces

A

forces of attraction between neighbouring molecules
forces that hold molecules together is solid or liquid state
much weaker then intramolecular forces

51
Q

what are the 3 types of intermolecular forces

A

London dispersion forces
Dipole- Dipole forces
hydrogen bonding

52
Q

what is london dispersion forces

A

attraction of a molecules electrons to neighbouring molecules protons
very temporary
larger the molecule larger LDF
EXIST IN ALL SUBSTANCES

53
Q

what is dipole dipole forces

A

electrostatic attraction between polar molecules
weaker then ionic ( partial charges)
MUST BE POLAR MOLECULE
PCl3

54
Q

what are vanderwaals forces

A

LDF and Dipole Dipole happening at the same time

55
Q

what is hydrogen bonding

A

extreme case of dipole dipole when hydrogen is bonded with O, N or F = VERY larger END
NOT A CHEMICAL BOND
strongest intermolecular force
h20

56
Q

what are chemical bonds

A

the forces of attraction holding atoms togther

57
Q

the octet rule

A

generalization stating that when atoms combime the combime so each atom achieves 8 valance electrons

58
Q

whats another name for ionic compounds

A

salts

59
Q

when can metals exist on their own

A

they are swimming in a sea of electrons

59
Q

how do intermolecular forces affect boiling point

A

Substances with strong intermolecular bonds have higher boiling points

60
Q

Difference between ionic molecular and anion

A

Ionic - crystal lattice negatives and positives
Molecular - sharing of electrons forms molecules
Anions- has a charge because of extra electrons ( charged molecule)

61
Q

Why do not all ionic compounds dissolve

A

Some ionic compounds electrostatic forces are stronger then the attraction between the anions and cation with the water so the crystal lattice doesn’t break into anions and cations

62
Q

Why does oil float on top of water

A

Water is more dense due to hydrogen bonding
Oil is a non polar molecule held by LDF which isn’t as strong as hydrogen bonding
Water isn’t attractive to the oil molecules only it’s self

63
Q

Why does ice float

A

Why ice forms hydrogen bonding force is strong it acts like a bond locking water molecules is crtystal lattice shape
Less dense because of orientation of water molecules ( big spaces)

64
Q

Why does ice float

A

Why ice forms hydrogen bonding force is strong it acts like a bond locking water molecules is crtystal lattice shape
Less dense because of orientation of water molecules ( big spaces)

Chemistry (3 decks)

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