Up and atom Flashcards
(81 cards)
1
Q
Atom
A
Smallest unit of an element retaining properties.
2
Q
Proton
A
Positively charged subatomic particle in nucleus.
3
Q
Neutron
A
Neutral subatomic particle in nucleus.
4
Q
Electron
A
Negatively charged subatomic particle in orbits.
5
Q
Atomic Number
A
Number of protons in an atom’s nucleus.
6
Q
Mass Number
A
Sum of protons and neutrons in nucleus.
7
Q
Nucleus
A
Central part of an atom containing protons and neutrons.
8
Q
Electron Configuration
A
Arrangement of electrons in an atom’s shells.
9
Q
Ion
A
Atom with a net positive or negative charge.
10
Q
Cation
A
Positively charged ion from losing electrons.
11
Q
Anion
A
Negatively charged ion from gaining electrons.
12
Q
Full Octet
A
Stable electron configuration with eight electrons.
13
Q
Periodic Table
A
Organized chart of elements by atomic structure.
14
Q
Subatomic Particles
A
Particles smaller than an atom: protons, neutrons, electrons.
15
Q
Natural Radioactivity
A
Decay of atomic nuclei releasing energy.
16
Q
Shells
A
Orbits around nucleus where electrons reside.
17
Q
Element
A
Substance made of identical atoms with unique properties.
18
Q
Experimental Evidence
A
Data supporting the development of atomic models.
19
Q
Proton Number
A
Determines the identity of an element.
20
Q
Particle Model
A
Explains behavior and arrangement of matter states.
21
Q
Electron Loss
A
Process where an atom loses electrons to become a cation.
22
Q
Electron Gain
A
Process where an atom gains electrons to become an anion.
23
Q
Atomic Model
A
Representation of atomic structure developed over time.
24
Q
Capacity of Shells
A
Maximum electrons each shell can hold.
25
Charge Neutrality
Condition where protons equal electrons in an atom.
26
Beryllium to Carbon Transition
Adding protons changes element identity from beryllium to carbon.
27
Which subatomic particle is positively charged
Proton
28
2. Which subatomic particle is negatively charged?
Electron
29
3. Name the subatomic particle that has no charge.
Neutron
30
3. Name the subatomic particle that has no charge.
Protons and Neutrons
31
4. Which two subatomic particles contribute to the mass of an atom?
PROTONS AND NEUTRONS
32
5. Which subatomic particle has the smallest mass?
ELECTRON
33
6. What occupies most of the volume of an atom?
The electron cloud
34
7. What determines the identity of an element?
The number of protons (atomic number)
35
8. How is the periodic table arranged in terms of atomic structure?
By increasing atomic number (number of protons) and electron configuration
36
9. An atom has 8 protons. How many electrons does it have? Explain why.
8 electrons – Because atoms are neutral, the number of electrons equals the number of protons.
37
10. An atom has a mass number of 7 and an atomic number of 3. How many protons and
neutrons does it have
3 protons, 4 neutrons – Mass number (7) = protons (3) + neutrons ⇒ 7 - 3 = 4
38
11. What is the mass number of an atom with 6 protons and 7 neutrons?
13 – 6 protons + 7 neutrons = 13
39
12. What is the charge of an atom if it has more electrons than protons?
Negative – More electrons than protons means extra negative charge.
40
13. What happens to an atom’s charge when it loses electrons?
It becomes positively charged – Because it loses negative electrons.
41
14. How many valence electrons do elements in Group 1 of the periodic table have?
1 valence electron
42
15. What does the period number in the periodic table indicate about an element’s
atomic structure?
Number of electron shells (energy levels)
43
16. What does the group number indicate about the element’s atomic structure?
Number of valence electrons
44
17. Why do atoms form ions?
To gain a full outer shell and become stable
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18. What is an isotope?
Atoms of the same element with different numbers of neutrons
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19. How do isotopes of the same element differ?
They have different masses (mass numbers)
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20. How are isotopes named?
Element name + mass number (e.g., Carbon-14)
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21. Define radioisotope
An isotope that is unstable and emits radiation
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22. Explain what happens during radioactive decay?
Unstable nuclei release particles or energy to become stable
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3. List the three types of radioactive decay
Alpha, Beta, Gamma
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24. What subatomic particles released during alpha decay and how many of each?
2 protons and 2 neutrons (a helium nucleus)
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25. Describe what happens to an atom when it undergoes alpha decay?
The atom loses 2 protons and 2 neutrons, forming a new element
53
26. State the process of beta decay?
A neutron changes into a proton and emits an electron (beta particle)
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27. How does beta decay affect an atom?
The atom gains one proton and changes to a different element
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28. Explain what occurs during gamma decay?
nucleus releases energy without changing the number of protons or neutrons
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29. Compare gamma rays to alpha and beta particles?
Gamma rays have no mass or charge and are more penetrating than alpha and beta
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30. List an example of a material that can stop each type of radiation?
Alpha – paper; Beta – aluminium; Gamma – thick lead or concrete
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31. State an example of an element that undergoes radioactive decay?
Uranium-238, Carbon-14, or Iodine-131
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32. Give three reasons why radioactive decay is important in science?
To date ancient materials (carbon dating)
For medical diagnosis and treatment
To understand nuclear reactions and atomic structure
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33. How do smoke detectors use alpha particles?
Alpha particles ionise air inside the detector; smoke disrupts this, triggering the alarm
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34. Explain carbon dating, and how does it work?
Carbon dating measures the decay of Carbon-14 in once-living things to estimate age
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35. How do X-rays and gamma rays help in medical imaging?
They pass through the body and create images of bones and organs
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36. Discuss how a PET scan works and explain its use.
A PET scan detects gamma rays from a radioactive tracer to show organ function
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37. How is radiation used to detect faults in aircraft and industry?
Radiation passes through materials to reveal cracks or faults
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38. Explain how radiotherapy is used to help treat cancer?
Radiotherapy uses radiation to kill or damage cancer cells
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39. State which type of radiation is commonly used in cancer treatment?
Gamma radiation
67
40. Define the term half-life mean?
The time it takes for half of a radioactive substance to decay
68
41. Explain how scientists use half-life to date fossils?
By measuring how much of a radioactive isotope is left in a sample
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42. State what nuclear fission is and how it generate energy?
Splitting a heavy nucleus releases energy; used in nuclear power plants
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43. State what nuclear fusion is and explain if it generates energy.
Joining light nuclei to form a heavier one; yes, it releases a lot of energy
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44. State where nuclear fusion occurs naturally?
In stars, including the Sun
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45. Einstein’s equation E=mc2 what does it mean?
Energy = mass × (speed of light)²; a small amount of mass gives a large amount of energy
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46. List some safety measures used to protect against radiation?
Wearing protective clothing
Using shielding (like lead)
Keeping distance and limiting exposure time
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47. Why is nuclear fusion considered a future energy source?
It produces more energy than fission
Has no long-term radioactive waste
Uses hydrogen, which is abundant
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Radioactivity
Decay of unstable atomic nuclei releasing energy.
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Alpha particles (α)
High-energy particles emitted from radioactive decay.
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Beta particles (β)
Electrons or positrons emitted during nuclear decay.
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Gamma radiation (𝛾)
High-energy electromagnetic waves from radioactive decay.
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Half-life
Time taken for half of a radioactive sample to decay.
80
Carbon dating
Method using carbon-14 to determine artifact age.
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