Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

physics- D > chem test > Flashcards

chem test Flashcards

1
Q

2 bonded atoms, 0 lone pairs

A

linear, 180, 2 total electron domains

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

domain

A

a location of a bond or a lone pair of electrons (double and triple bonds only count as one domain)

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

3 bonded atoms, 0 lone pairs (Boron triflouride; BF v 3)

A

trigonal planar, 120, 3 total electron domains

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

2 bonded atoms, 1 lone pair (Nitrate Ion; NO v 2 ^ -1)

A

bent, 118, 3 total electron domains

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

4 bonded atoms, 0 lone pairs (Methane; CH v 4)

A

tetrahedral, 109.5, 4 total electron domains

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

3 bonded atoms, 1 lone pair (Ammonia; NH v 2)

A

trigonal pyramidal, 107, 4 total electron domains

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

2 bonded atoms, 2 lone pairs (water; H v 2 O)

A

bent, 104.5, 4 total electron domains

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

5 bonded atoms, 0 lone pairs (PCl v 5; Phosphorus pentachloride)

A

trigonal bipyramidal, 120 and 90, 5 total electron domains

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

6 bonded atoms, 0 lone pairs (Sulfur nexaflouride; SF v 6)

A

octahedral, 90, 6 total electron domains

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

diatomic ions, and what elements can form them

A

ions made up of two atoms of the same element. They are always found together in a compound. The following elements can form diatomic ions: H, N, O, F, Cl, Br, and I.

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

monatomic ions

A

are ions formed from a single atom. They can be either positive or negative.

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

cation

A

ion that has lost electrons and has a positive charge (cat–> PAWsitive)

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

anion

A

ion that has gained electrons and has a negative charge

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

ion

A

An ion is an atom or a group of atoms that has gained or lost electrons, resulting in a positive or negative charge

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

what follows single element cations? for example Na ^ +

A

the name of the element is used followed by the word word “ion”
Na ^ + = sodium ion

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

what follows single element anions? for example Cl ^ -

A

the name of the element is used followed by the suffix “-ide”
Cl ^ - = chloride ion

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

how do you write a single element transition metal ion? for example Fe ^ 3+

A

you have to include the charge in roman numerals following the element name
Fe ^ 3+ = iron (III) ion

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

NH v 4 ^ +

A

ammonium

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

SO v 3 ^ 2-

A

sulfite

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

SO v 4 ^ 2-

A

sulfate

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

OH -

A

hydroxide

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

PO v 4 ^3 -

A

phosphate

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

O v 2 ^2 -

24
Q

how do you write and name ionic bonds? for example Na+Cl-

A

criss cross their charges down (to achieve neutrality)
Subscripts must be the lowest ratio when canceling charges.
positive metal ion always comes first
drop the second syllable of the negative/anion element and subsitute with “-ide”
Na+Cl- = NaCl
sodium + chlorine = sodium chloride

25
ionic compounds must have an overall ______ charge
neutral (charge of 0)
26
what are ionic compounds made of?
- Ionic compounds are formed when positive and negative ions combine. - have a metal and a nonmetal
27
how do you name transition metal ionic compounds? for example CuO vs Cu v 2 O
you include the roman numeral in the name CuO = copper (I) oxide Cu v 2 O = copper (II) oxide
28
polyatomic ions
most polyatomic ions are covalent ions that are made with more than two elements (SO v 4 ^ 2- = sulfate) - when you do the drop and switch (criss cross), use parenthesis ex: Ca ^ 2+ + NO v 3 ^ -1 = Ca(NO v 3) v 2 use both names --> calcium nitrate if there are two polyatomic you use both of them as well --> ammonium oxalate
29
ionic compounds with transition metals; for example Cu ^ +2 Cl ^ -1
CuCl v 2 = copper (II) chloride make sure to specify the charge of the transition metal with roman numerals (re criss crossing )
30
covalent compounds are made of ______
two or more nonmetals SHARE electrons
31
how do you name covalent bonds? for example SO
prefixes are used to indicate the number of atoms in each element - end second element with "-ide" - mono is NOT used for the first element - sulfur monoxide
32
prefixes
1- mono 2- di 3- tri 4- tetra 5- penta 6- hexa 7- hepta 8- octa 9- nona 10- deca
33
VSEPR
valence shell electron pair repulsion - The model states that electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible. - VSEPR theory allows more accurate predictions of molecular shape
34
intermolecular
attractive force between molecules (dipole= polarity)
35
different types of IMF (intermolecular forces) put them from strongest to weakest
hydrogen bonding dipole-dipole attraction london dispersion attraction
36
dipole-dipole attraction
occurs between : partially oppositely charged ions relative strength: strong
37
hydrogen bonding
occurs between : H atom and O, N or F atom relative strength: strongest of the dipole- dipole attraction
38
london dispersion attraction
occurs between: temporary or induced dipoles relative strength: weakest
39
metallic bond diagram
sea of e- (reason for conductivity)
40
lone pair
a pair of valence electrons that are not shared between atoms (aka nonbonding pair or unshared pair )
41
single pair
bond between two atoms by one pair of electrons
42
double pair
bond between two atoms by two pairs of electrons
43
triple bond
bond between two atoms by 3 pairs of electrons
44
what type of bond are H v 2 O NaCl
H v 2 O = bent because it has one bond - covalent, polar NaCl = linear because it only has 2 pairs - ionic
45
types of covalent bond types
polar and nonpolar
46
polar
typically between two different elements - electrons are more on one side than the other (toxic bf) Sharing of electrons: unequal attraction for electrons so the sharing is UNEQUAL electronegativity difference: 0.4-1.7 _____> examples: HF H F
47
non polar
Sharing of electrons: shared equally between the two atoms Electronegativity difference: less than 0.4 examples: Cl Cl-----> Cl v 2
48
octet rule
atoms prefer to have 8 electrons in the valence shell
49
lewis dot diagrams
- atomic models which show valence electrons and can be used to predict bonding - bonding occurs when atoms try to reach octet
50
ionic compound (characteristics)
- lattice structure of atoms, transfer of electrons conductivity: electrons are FIXED, no conductivity in solids, conductivity in liquid solubility: many are soluble in H v 2 o state of matter: crystaline solids other: large electronegativity difference between ions (greater than 1.7) electrons: transferred from metal to non-metal. elements attracted by opposite charges
51
covalent compound (characteristics)
- sharing of electrons conductivity: no conductivity solubility: most are non soluble in H2O, soluble in nonpolar solvents state of matter: liquid or gas at room temperature other: small or no difference in electronegativity between atoms (less than 1.7: polar 0.4-1.7; non-polar 0-0.4) electrons: shared between 2 nonmetals
52
Metallic compound (characteristics)
- sea of electrons (e-) conductivity: good conductivity solubility: most do not dissolve in H2O, some react with H2O state of matter: solid at room temperature, mercury at room temp is a liquid other: most metallic bonds are made of the same atoms so electrons are shared equally - alloys are mixtures of metals
53
alloys
mixtures of metals
54
electronegativity
the tendency of an atom to attract electrons to itself in a chemical bond
55
what occurs when salt dissolves in water?
the molecules mix amongst eachother
56

physics- D (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions