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Chemistry game 2018 Flashcards | StudBud
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Chemistry game 2018
Chemistry game 2018
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Chemistry game project. 2018
Flashcards
95 cards
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Answers
1
Chapter 2
Section 7: what is the temperature formula for F° to C°?
5/9=C
(F-32)•5/9=C
F-32•C
F•5/9=c
2
Chapter 6
Section 2:What do we use chemical equations for?
chemicals present before the reaction and after the reaction
Present chemicals and that's all
Reaction chemicals
To name them
3
chapter 8
Section 6: What’s the difference between molecular and empirical formulas?
molecular tells you reduced ratio of elements
Molecular tells how many atoms of element are in a compound
empirical says how many atoms are in an element compound
empirical says most reduced ratio of elements in a compound.
4
chapter 4
Section 10: Define IONS
Loss of electrons
I don't know
Gain of electrons
molecule with a electric charge, loss or gain of electrons.
5
chapter 8
Section 8: How to calculate molecular formula
get formula, get mass
find empirical formula, get mass, convert mass to mole,ratio
find ratio, mass to mole
get mass ,convert mole
6
Chapter 2
Section 5: are zeros significant?
Any zeros between two significant digits are significant.
trailing zeros in the decimal portion only are significant.
Non-zero digits are always significant.
All of the above
7
chapter 7
Section 5: What is an Oxidation-Reduction reaction?
form mixtures
A transfer of electrons in a reaction.
reduce oxidation
Compose bonds
8
chapter 13
Section 1: Name the 3 stages of water
Solid
liquid
gas
all of the above
9
chapter 7
Section 3: Name two types of equations
bonding components
Molecular
balancing equations
Net Ionic
10
Chapter 4
Section 9
:
How many of the elements are naturally occurring?
19 elements
t 90 elements occur naturally.
92 elements
95 elements
11
chapter 10 Section 11: list main atomic trends
electronegativity, ionization energy, electron affinity
atomic radius, melting point, and metallic character.
Just A
Both a and b
12
chapter 5
Section 2: Whats the name for naming metal and non-metal compounds?
double displacement
Ionic compounds
Periodtic table
Compounds
13
Chapter 6
Section 1
:
Give three examples of a chemical reaction occurring/occurred
color, physical form, bubbles
Rust, fire, bubbles
smell, taste, feel
bubbles, fire, color
14
Chapter 3
Section 3
:
what are elements and what are compounds?
Elements can’t be broken down into other substances
Compounds can be broken and are bonded together.
I don't know
Bonds
15
Chapter 2
Section 3: what is an example(s) of a metric unit for mass, length, and volume?
meters
grams
liters
pounds
16
Chapter 4
Section 5:What are three compound stat make up an atom?
i don't know
Neutrons, electrons, Protons
Elements, electrons, hydrgen
Funds, grams, ounces
17
chapter 5 section 4
Name two types of ionic compounds
Binary Ionic compounds
binary type two
both
18
Chapter 2
Section 2:
What are the two main Units used today?
Metric unit And Standard or English unit
I don't know
Pounds, cups, tablespoon
Kilograms, meters, grams
19
Chapter 11
Section 2: how to use the periodic table
Look up symbols for the element needed
In rows and goups
Just guess
20
chapter 7
Section 6: Name other ways to classify reactions
All of the above
Oxidation Reduction.
Acid Base.
Double Displacement
21
chapter 7
Section 4: How did Arrhenius define acid and bases?
Bases are a substance that produces hydroxide ions in water.
Acids produce H+ Ions when dissolved in water.
Both
22
What is the difference between Qualitative and Quantitative? Chapter 1 section 3
Numbers and observations
Quantitative is numerical,Qualitative is on observations.
I don't know
Quantitative is observations, Qualitative is numerical
23
chapter 4
Section 11:Name two of the Ionic compound properties
They form crystals
Brittle
High melting and boiling points
They are hard
24
chapter 12
Section 8: Kinetic molecular theory name one
Gas particles undergo no molecular attractions or repulsions
Gas particles are in continuous, random motion
all of the above
gases have no volume but have defined mass
25
chapter 10
Section 9:name three types of electron configuration
box diagrams
abbreviated
All of the above
regular,
26
chapter 8 Section 4: Define molar mass-
I
A property of elements
the molar mass M is property defined as mass of a substance
Atomic mass of an element
27
chapter 5 Section 3: What is compounds that only contain nonmetals called?
single displacement
ionic compounds
Covalent compounds
covalent bonds
28
chapter 4
Section 6:
What are the charge for protons, electrons, and neutrons?
All of the above
neutrons have no charge
Protons are positive
electrons have negative charge.
29
chapter 15
Section 4: What is the ph scale used for?
represents bases
shows levels of element
provides a convenient way to represent solution acidity.
30
Chapter 2 Section 1:
What is the scientific notation used for?
Numbers in decimal form
express numbers that are big/small to be in decimal form.
Express whole numbers
I don't know
31
chapter 5 section 5
What does polyatomic ions do in compounds?
Charge entity composed of several atoms bound together.
charge only 2 atoms
none of the above
charge ions only
32
Chapter 3
Section 4:define what mixture and pure substances are
-
Mixes are hetero./ homo.can separate to original substances.
Pure substances are compounds or elements are consistent.
elements
Bonded
33
Chapter 4
Section 3A: What is the law of conservation?
any system closed to all transfers of matter and energy
quantity cannot be added or removed.
the mass of the system must remain constant over time
i don't know
34
Chapter 11
Section 1:Define bonding
a chemical bond that attracts between atoms and ions
A physical bond that attracts bonds
Atoms and Ion attracted mixtures
35
What are the scientific method steps? Chapter 1 section 2
Communicate, analyze, test, hypothesis, research, question
Question,research,Hypothesis,Test, Analyze, Communicate
research,test,analyze,question,hypothesis
test, question, hypothesis, research
36
chapter 14
Section 5 Define Dilution
the action of making a liquid more dilute.
to boil something
to melt something
to vaporize something
37
Chapter 4
Section 1: Name elements on the periodic table
Iron
Calcium
Tin
Nitrogen
38
chapter 11
Section 7:
define multiple bonds
all of the above
multiple bond is where protons are converted by an atom
multiple bond is where neutrons are converted by an atom
multiple bond is electrons that are converted by an atom.
39
chapter 11
Section 6:
how to set up the Lewis structure
Element with 9 dots around it
the element then in sets of twos, dots all round it
None of the above
element with several dots
40
chapter 5
Section 7
:
Give an example of an formula
C6H12O6
H202
CH4
NH3
41
chapter 10
Section 10 : Define electronic configurations
the arrangement of neutrons
The arrangement of electrons in the orbitals of an atom
The arrangement of protons in an atom
the arrangement of mixtures
42
chapter 14
Section 2: Name the quantitative descriptions of solutions
concentrated
all of the above
Dilute
unsaturated, saturated
43
chapter 5
Section 6: How to name acids :
Periodic table
Ic at the end
Tasting them
“hydro-“, ending in “-ic”, if ends in "ate" "ic" replaces it
44
chapter 11
Section 4: what is the stable electronic configuration used for?
All elements
None
main groups or noble gases
Just Hydrogen
45
chapter 15 Section 3: Explain amphoteric substance of water
all of the above
energy transfer to one molecule to another
water transfer to one electron to another
transfer of a proton from one water molecule to another
46
chapter 10
Section 6: wave mechanical model atom definition-
an atom with only neutrons
An atoms only contains electrons
an atoms with protons and neutrons
the atom contains protons/neutrons surrounded by electrons
47
Chapter 5 Section 1:Why is it necessary to name compounds?
To name them
For chemistry
To see if the compounds are metal or nonmetal
48
chapter 12
Section 4: avogadro’s law-
Pv=nrt
V1/T1=V2/T2
V1 / n1 = V2 / n2
P1 X V1 = P2 X V2
49
CHAPTER 12
.Section 5: Ideal gas law
V1 / n1 = V2 / n2
V1/T1=V2/T2
P1 X V1 = P2 X V2
Pv=nrt
50
chapter 4 section 7
Define Isotopes
i don't know
forms of same element that contain same numbers of protons
Different numbers and different elements
51
chapter 15
Section 5: what is the calculation method to find PH of a strong acid?
-log[H+]
- pH = -Log[H+]
none of the above
-PH=-log
52
chapter 11 .Section 3: what is dipole
dipole moments happen during mixtures
Dipole moments happen during just separation
All of the above
dipole moments occur when there is a separation or charge
53
chapter 13
Section 2: What happens to matter when energy is added?
Adding energy to matter causes a physical change
no change
changes slightly
causes chemical change
54
chapter 6
Section 3:
how do you balance a chemical equation?
use compounds
Reactants -->products
Products --> reactants
55
Chapter 2
Section 8:define density
Ratio of units
It's the ratio between mass and volume or mass per unit
Units
Mass and volume
56
chapter 10
Section 7:what do the letters stand for
Both a and b
sharp, principal,
diffuse, fundamental
57
chapter 8
Section 5:what is percent composition-
the percent of compounds
The percent of units
Percent com. is mass of each element present in a compound.
the percent of mixtures
58
chapter 12
Section 10: define gas stoichiometry
quantitative relations between reactants products chemically
quantitative relations between chemicals
none of the above
relation between elements
59
chapter 7
Section 2: What is a precipitation reaction?
when reactions forms a gas
When the reaction is the formation of a solid
when reaction forms a liquid
when reaction forms a element
60
Chapter 4
Section 2:What are the element symbols for tin, iron, nitrogen, calcium
I,O,H,Te
At,Rn,O,Pd
Eu,U,Cs,Fr
Sn,Fe,N,Ca
61
chapter 14
Section1: How does solubility dissolves like
None of the above
nonpolar solutes can dissolve in nonpolar solvents.
polar solutes can dissolve in polar solvents
Both A and B
62
chapter 8
Section 1: Why do we count by weighing
All of the above
saves time for the rest of the experiment
To get an over all weight of several things
63
Chapter 3
Section 7:What is the formula for energy and heat
?
joules
Heatxmass
Heat transfer =(mass)(specific heat)(temperature change)
i don't know
64
chapter 9
Section 3: how to get mass to mass ?
must use formulas
Must use stoichiometry
must use compounds
65
Chapter 2
Section 6: how many steps are there in the metric unit conversion?
2, G-G, M-G
6, G-G, G-G ,G-M, G-M, M-M, M-M
4, g-g,g-m,m-m,m-g
3 , M-M, M-G, G-G
66
chapter 14
Section 3: how to find mass percent
Divide the mass by the total mass and multiply by 100.
all of the above
100 = total mass
divide the mass by 100
67
chapter 16
Section 2:what are some factors that influence reaction rates?
none of the above
Catalyst enzymes and the activation energy levels.
just energy
just catalyst
68
Chapter 4
Section 3:What are three points dalton made?
Atoms are cool
All atoms of an element are identical
Atoms of different elements vary in size and mass.
Everything is composed of atoms
69
chapter 7
Section 7: Three classify reactions
Single replacement,
Combustion
Synthesis
decomposition.
70
Chapter 4
Section 4:What are chemical formulas used for?
To use for fun
Labeling and that's all
Symbols
It’s the chemical proportions stated with symbols, numbers.
71
Chapter 12
Section 6: Dalton’s law of partial pressure
pressure is equal to itself
all of the above
Pressure is equal to mass
the pressure exerted is equal to individual gases
72
chapter 9
Section 4: What is a limiting reactant?
the reactant to the the product
the substance that is consumed, then the experiment is over
The reactant to cause the experiment
73
chapter 9
Section 2: How to get mole to mole ratios
Must use a balance equation
have to use compounds
have to use mixtures
74
chapter 10
Section 3:when do atoms emit light?
When the atoms are tired and are sleeping
when the atoms get excited and get energy.
when the atoms separated
when the atoms turn on a lamp
75
chapter 7
Section 1: What are driving forces of reactions?
Combustion bonds
Gases
Double replacement, combustion, and decomposition
76
chapter 1 section 1 What is Chemistry?
The universe
chemicals
Science that deals with objects and their properties/changes
I Don't know
77
Chapter 9
.Section 5: Define percent yield
percent of compunds
the percent ratio of actual yield to the theoretical yield.
Percent of the elements
percent of mixtures
78
chapter 8
.Section 2: What do we use to count atoms -
Units
Formulas
Atomic mass
Compounds
79
chapter 8
Section 7: how to calculate empirical formula
round to whole and divide grams
mass to moles, divide and round
convert, and divide
grams ,Convert the mass to moles Divide,Round to whole
80
chapter 14
Section 4: How to find molarity
m= solvent
m= elements
M=Solute over solution
m= produce
81
CHAPTER 12 Section 3: charles law
v1/t1=v2/t2
V1 / n1 = V2 / n2
P1 X V1 = P2 X V2
Pv=nrt
82
chapter 10
Section 5: What does the bohr model show
Protons orbiting around nucleus
Neutrons orbiting around nucleus
Electrons in atoms orbiting offering energy around nucleus
83
Chapter 3
Section 5:How to separate mixtures
a funnel
evaporation
Filtration
distillation
84
chapter 12 Section 2: boyle’s law
V1 / n1 = V2 / n2
V1/T1 =V2/T2
P1 X V1 = P2 X V2
Pv=nrt
85
chapter 9
Section 1: Information given by a balanced equation-
i don't know
chemical equation will get formulas and symbols/products
Will get you products
86
Chapter 4
Section 8:How many groups are there on the periodic table?
22 groups
19 groups
18 groups
30 groups
87
chapter 8 section3
What unit does avogadro's law use?
Avogadro's number, units in one mole of any substance
boyle's law
standard method
metric unit
88
Chapter 3
Section 1: Name the three states of matter
pounds, grams, units
gas, grams, ounces
Solid, Liquid, and gas
Solid, gas, oxygen
89
chapter 10
Section 8: What does the pauli exclusion principle say about electrons
only 1/2 of an atom can exist in an atom
Only 1 electron can exist in any particular state in a atom
All of the above
2 electrons can exist in an atom
90
chapter 12
Section 1: Define pressure -
continuous physical force on or against an object
none of the above
build up of water
91
Chapter 3
Section 6: What are the definitions of energy and heat
i don't know
Energy
a form of energy transfer among particles in a substance.
Heat energy is also called thermal energy or heat.
92
chapter 15
Section 1: define acids and bases
bases remove water, acids are h20
acids neutralizes alkalis. Bases release hydroxide ions
none of the above
acids are alkalis
93
Chapter 3
Section 2:Explain what a physical and chemical property is
Characteristics
Physical is characteristics, Chemical forming new substance
i don't know
Not noticeable changes
94
chapter 10
Section 4:what do the energy levels make the atom of hydrogen do?
go side to side
Stand still
Dance
makes them go up and down
95
chapter 10
Section 2: how do we use electromagnetic radiation?
x Rays
All of the above
microwaves
radio waves.
