stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
MEASUREMENTS AND ATOMS Flashcards | StudBud
Explore
/
MEASUREMENTS AND ATOMS
MEASUREMENTS AND ATOMS
35 terms
·
StudBud Administration
·
51 plays
Imported from external platform
Flashcards
35 cards
F
Practice quiz
P
Host live
L
Questions
35
Answers
1
On a dartboard, all darts hit the bullseye. This demonstrates ___________.
Both accuracy and precision.
Precision only.
Accuracy only.
Neither accuracy nor precision.
2
Which of the following materials is likely to have the highest density?
Lead
Sugar
Aluminum
Water
3
Dalton’s Atomic Theory explains why _______.
Compounds always contain the same ratio of elements.
Atoms cannot be divided further by chemical means.
Elements cannot change into other elements during chemical reactions.
All of these
4
What is the best definition of "precision"?
The closeness of a measurement to the true value.
The reduction of systematic errors.
The closeness of measurements to one another.
The ability to achieve consistent accuracy.
5
If different groups record widely varying results for the same experiment, it indicates low ________.
Accuracy
Precision
Reliability
Consistency
6
If an atom of carbon has 6 protons, 6 electrons, and 7 neutrons, which isotope is it?
Carbon-12
Carbon-15
Carbon-13
Carbon-14
7
According to the Law of Multiple Proportions, if two elements form more than one compound ____________.
The compounds have different physical states.
The compounds have identical properties.
Their masses are always equal.
The ratios of their masses in the compounds are whole numbers.
8
What is an ion?
A molecule made of charged particles
An atom that has gained or lost protons
A particle that contains only neutrons
An atom that has gained or lost electrons
9
The mass number of an atom is the total number of protons and electrons in the nucleus.
False
True
10
Who is credited with formulating the Law of Conservation of Mass?
Joseph Proust
John Dalton
Antoine Lavoisier
Dmitri Mendeleev
11
The number of electrons in a neutral atom is equal to the number of protons.
True
False
12
If the density of an object is less than the density of the liquid it is placed in, the object will ___________.
Disappear
Sink to the bottom
Remain suspended in the liquid
Float
13
Which experiment led to the discovery of the nucleus?
J.J. Thomson’s cathode ray experiment
Rutherford’s gold foil experiment
Millikan’s oil drop experiment
Chadwick’s neutron experiment
14
An atom with an atomic number of 15 and a mass number of 31 has how many neutrons?
46
31
15
16
15
Which subatomic particle is least likely to influence the mass of an atom?
Neutron
Electron
Positron
Proton
16
What happens when an atom gains an extra electron?
It becomes neutral.
It loses its protons.
It becomes negatively charged.
It becomes positively charged.
17
Which of the following best describes isotopes of the same element?
They have the same number of protons but different numbers of neutrons.
They have the same number of electrons and neutrons.
They have different numbers of protons but the same number of neutrons.
They have different chemical properties.
18
What is an anion?
An ion with a positive charge
A molecule with a negative charge
An ion with a negative charge
A neutral atom
19
Whose model was shown in the picture?
J.J. Thomson
James Chadwick
Ernest Rutherford
Niels Bhor
20
Which scenario is an example of precision?
Getting results of 2.5 mL, 2.6 mL, and 2.4 mL in three trials.
Obtaining values that match expected results.
Continuously hitting the center of a target.
Measuring the boiling point of water as exactly 100°C.
21
The isotope iodine-131 is primarily used for __________.
Treating thyroid disorders
Carbon dating
Diagnosing fractures
Sterilizing medical equipment
22
Which law explains why water is always composed of hydrogen and oxygen in a 2:1 ratio by mass?
Law of Definite Proportions
Law of Conservation of Mass
Dalton’s Atomic Theory
Law of Multiple Proportions
23
The Law of Definite Proportions states that _____________.
Matter is made up of small, indivisible particles.
Compounds are always made of the same elements in fixed ratios by mass.
The total mass of reactants equals the total mass of products.
Atoms combine in random proportions to form compounds.
24
Dalton’s Atomic Theory states that ____________.
All of these
Atoms of the same element are identical in all respects.
Atoms are indivisible and cannot be destroyed.
Atoms combine in simple whole-number ratios to form compounds.
25
Dalton’s Atomic Theory replaced which earlier idea?
Democritus’ concept of indivisible particles
The phlogiston theory
Lavoisier’s conservation of mass
Rutherford’s nuclear model
26
Which of the following particles does
NOT
contribute to the charge of an atom?
Neutron
Proton
Positron
Electron
27
Which of the following is
NOT
a fundamental law of chemistry?
Law of Thermodynamics
Law of Conservation of Mass
Law of Multiple Proportions
Law of Definite Proportions
28
Isotopes of an element always have the same chemical properties because they have the same number of electrons.
True
False
29
Which of the following best describes the Law of Conservation of Mass?
Matter can be created but not destroyed.
Energy can be converted into matter.
Mass and volume are conserved in all chemical reactions.
The mass of reactants is always equal to the mass of products.
30
If two objects have the same mass but different volumes, which one will have a higher density?
Cannot be determined
Both will have the same density
The one with a smaller volume
The one with a larger volume
31
If a substance has a mass of 50 g and a volume of 10 cm³, its density is _________.
5 g/cm³
500 g/cm³
50 g/cm³
0.5 g/cm³
32
Whose model was shown in the picture?
Ernest Rutherford
James Chadwick
J.J. Thomson
Niels Bhor
33
What is the formula for density?
Density = Volume × Mass
Density = Volume ÷ Mass
Density = Mass ÷ Volume
Density = Mass × Volume
34
If a thermometer consistently shows temperatures 3°C higher than the actual value, it can be described as _______.
Precise but not accurate.
Neither accurate nor precise.
Both accurate and precise.
Accurate but not precise.
35
Which ion does chlorine typically form?
Cl⁻
Cl⁺
Cl³⁻
Cl²⁻
