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Elements atoms periodic table answers

 

 

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Elements atoms periodic table answers

 

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Chemistry

 

Elements atoms periodic table answers

 

Elements, Atoms, and the Periodic Table

True/False

 

1. The mass number of an atom is the sum of the numbers of protons and neutrons in the nucleus.

True; Easy

2. There are 90 man made elements known today.

False; Easy

3. Helium is the most abundant element in the universe.

False; Easy

4. Oxygen is the most abundant element on the earth and the second most abundant in the universe.

False; Easy

5. The relative amounts of elements in our body are directly proportional to their abundances on Earth.

False; Easy

6. ‘Sn’ is the chemical symbol for strontium.

False; Moderate

7. The chemical symbol for manganese is ‘Mn.’

True; Easy

8. Modern atomic theory states that an electron is the smallest part of an element that maintains the identity of that element.

False; Moderate

9. The electron was the first subatomic particle to be discovered, and has a mass of 9.109 ´ 10−31 kg.

True; Easy

10. A proton and a neutron have almost the same mass.

True; Moderate

11. Rutherford’s experiments showed some alpha particles that were deflected straight back, indicating that electrons were concentrated in the nucleus.

False; Moderate

12. Particles in the nucleus have negative charge.

False; Moderate

13.  The orbiting electrons in an atom account for its size.

True; Easy

14. In Rutherford’s experiments, the deflection of some alpha rays prove that an atom is mostly empty space.

False; Moderate

15. In a neutral atom, the number of protons equal the number of electrons.

True; Moderate

16. Isotopes have the same mass number but a different atomic number.

False; Moderate

17. The mass of one carbon atom in atomic mass units is 12 u.

            True; Moderate

18. The electronic configuration of silicon is 1s22s22p63s22p2.

True; Moderate

19. Elements in the same column will have similar chemical properties.

True; Easy

20. Increasing the number of electrons in a given shell of an atom will increase the atomic radius of that atom.

            False; Moderate

 

Multiple Choice Questions

21. Which of is the most abundant element in the universe?

• Helium
• Oxygen
• Hydrogen
• Silicon
• Iron

c; Easy

22. Which is the most abundant element present in Earth?

• Oxygen
• Silicon      
• Aluminum
• Iron
• hydrogen

d; Easy

23. What is the chemical symbol for copper?

• Co
• Cp
• Ce
• Cr
• Cu

e; Easy

24. The symbol of which of the following elements comes from its German name—wolfram?

• Zirconium
• Strontium
• Platinum
• Lithium
• Tungsten

e; Moderate

25. The chemical symbol for silver is derived from _____.

• arsenic
• aurum
• argentum
• aluminum 
• armenium

c; Easy

26. What is the chemical symbol for sodium?

• Su
• So
• S
• Ni
• Na

e; Moderate

27.  The chemical symbol ‘Sn’ stands for _____.

• strontium
• sodium
• silicon
• titanium
• tin

e; Moderate

28. Which of the following is an element?

• Wood
• Juice
• Air
• Iron
• Liquefied CO2

d; Easy

29. What is the correct chemical symbol for cobalt?

• Ct
• CB
• Cb
• Co
• C

d; Easy

30. Which of the following elements exist as a diatomic molecule?

• Iron          
• Neon
• Iodine
• Carbon
• Calcium

c; Moderate

31. What does the modern atomic theory state?

• All elements are composed of molecules.
• All molecules are composed of atoms.
• All elements are composed of atoms.
• All compounds are composed of molecules.
• All atoms are of the same size.

c; Moderate

32. Which of the following was an incorrect assumption made by Dalton?

• Elements are composed of atoms.
• Compounds are composed of molecules.
• All matter is composed of atoms.
• Atoms cannot be divided further.

e.    Atoms are of differing sizes.
d; Easy

33. Atoms are composed of _____ different kinds of particles.

• one
• two
• three
• four
• six

c; Easy

34. What common quantity do electrons and protons share?

• Size
• Mass
• Position
• Charge     
• Energy

d; Moderate

35. What is the mass, in kg, of a neutron?

• 1.673 × 10 – 27
• 9.109 × 10 – 31
• 1.675 × 10 – 27  
• 9.109 × 10 – 27
• 1.675 × 10-31

c; Moderate

36. An alpha particle, a positively charged particle, is a combination of _____.

• two protons and two neutrons
• two electrons and two protons
• two neutrons and two electrons
• one proton and two electrons
• two electrons and one neutron

a; Easy

37. What did Rutherford conclude about the internal structure of an atom?

• Electrons and neutrons are concentrated in the nucleus.
• Protons and electrons are concentrated in the nucleus.
• Only electrons are present in the nucleus.
• Only neutrons are present in the nucleus.
• Protons and neutrons are present in the nucleus.

e; Moderate

38. In Rutherford’s experiments, most of the alpha particles traveled through the metal foil. Which of the following does this indicate?

• Protons are present in the nucleus.
• Neutrons are present in the nucleus. 
• An atom consists largely of empty space.
• Electrons orbit the nucleus.
• Protons are positively charged.

c; Easy

39. Which of the following is the smallest?

• A hydrogen atom
• A hydrogen nucleus
• An electron
• A helium atom
• A helium nuclei

c; Moderate

40. Which of the following is the biggest?

• A proton
• A neutron
• An electron
• A helium nuclei
• A helium atom

e; Easy

41. If an atom is electrically neutral, then:

• the number of electrons equals the number of neutrons.
• the number of neutrons equals the number of protons.
• the number of electrons equals the number of protons.
• there are fewer number of electrons than protons.
• there are fewer number of protons than electrons.

c; Easy

42. The atomic number of an atom is equal to:

• the number of neutrons and electrons in an atom.
• the number of electrons in an atom.
• the number of neutrons in an atom.
• the number of protons in an atom.
• the number of neutrons and protons in an atom.

d; Easy

43. How many electrons are present in a neutral atom of carbon? (Hint: The atomic number of carbon is 6.)

• 12
• 6
• 3
• 18
• 9

b; Moderate

44. What are isotopes?

• Atoms of an element with different number of electrons.
• Atoms of an element with different number of protons.
• Atoms of an element with different number of neutrons.
• Atoms of an element with different atomic numbers.
• Atoms of an element with different number of nuclei.

c; Moderate

45. A neutral atom of hydrogen has a single electron and a single neutron. What is its atomic number and mass number? 

• 1 and 1
• 1 and 0
• 1 and 3
• 1 and 2
• 0 and 1

d; Easy

46. Which of the following statements is true of?

• 56 is the number of electrons in iron.
• 56 is the number of protons in iron.
• 56 is the number of neutrons in iron.
• 26 is the number of protons in iron.
• 26 is the number of neutrons in iron.

d; Moderate

47. What is the number of neutrons in?

• 8
• 6
• 12
• 2
• 14

a; Moderate

48. What iscalled?

• Hydrogen
• Cesium
• Deuterium
• Osmium
• Tritium

e; Moderate

49. How many neutrons does U-238 have?

• 98
• 238
• 236
• 146
• 144

d; Easy

50. What is an atomic mass unit?

• The mass of twelve carbon atoms.
• The mass of one carbon atom.
• The mass of one hydrogen atom.
• One twelfth of the mass of one carbon atom.
• The mass of twelve hydrogen atoms.

d; Moderate

51. If 90% of an element ‘E’ exists as and 10% as , then its atomic mass would be _____?

• 21 u
• 24 u
• 21.3 u
• 22.4 u
• 45 u

c; Moderate

52. What is the average mass of an oxygen atom in grams? (Atomic mass of oxygen = 15.994 u)

• 2.657 × 10 – 23  g
• 16 g
• 15.995 g
• 8 g
• 26.57 × 10 – 23 g

a; Moderate

53. Electrons are organized according to their energies into sets called _____.

• shells
• orbits
• cellars
• quanta
• levels

a; Moderate

54. Which of the following has the biggest atomic radius?

• Argon
• Bromine
• Chlorine
• Phosphorus
• Sulfur

b; Moderate

55. Which of the following represent the four subshells that make up a shell?

•  s, p, d, f
• a, b, c, d
• p, q, r, s
• k, l, p, d
• s, p, e, d

a; Moderate

 

Essay

56. Write a brief note on elements.

An element is a substance that cannot be broken down into simpler chemical substances. There are about 90 naturally occurring elements known on Earth. Using technology, scientists have been able to create nearly 30 additional elements that do not occur in nature. Today, chemistry recognizes 118 elements—some of which were created an atom at a time.
Easy

57. Describe the abundance of elements in the universe and on Earth.

The elements vary widely in abundance. In the universe as a whole, the most common element is hydrogen (about 90% of atoms), followed by helium (most of the remaining 10%). All other elements are present in relatively minuscule amounts, as far as we can detect.
On the planet Earth, however, the situation is rather different. Oxygen makes up 46.1% of the mass of Earth’s crust (the relatively thin layer of rock forming Earth’s surface), mostly in combination with other elements, while silicon makes up 28.5%. Hydrogen, the most abundant element in the universe, makes up only 0.14% of Earth’s crust.
Easy

58. Briefly describe the chemical symbol for elements.

By convention, the first letter of a chemical symbol is a capital letter, while the second letter (if there is one) is in lowercase. The first letter of the symbol is usually the first letter of the element’s name, while the second letter is some other letter from the name. Some elements have symbols that derive from earlier, mostly Latin names, so the symbols may not contain any letters from the English name.
Easy

59. Briefly describe the three subatomic particles?

The first subatomic particle was identified in 1897 and called the electron. It is an extremely tiny particle, with a mass of about 9.109 × 10− 31 kg. Experiments with magnetic fields showed that the electron has a negative electrical charge. A proton has the same amount of charge as an electron, but its charge is positive, not negative. Another major difference between a proton and an electron is mass. Although still incredibly small, the mass of a proton is 1.673 × 10−27 kg. The neutron is a particle with about the same mass as a proton but with no electrical charge.
Easy

60. Describe the setup of Rutherford’s Gold leaf experiment.

Rutherford and his colleagues took a very thin metal foil, such as gold or platinum, and aimed a beam of positively charged particles (called alpha particles) from a radioactive source toward the foil. Surrounding the foil was a detector—either a scintillator (a material that glows when hit by such particles) or some unexposed film (which is exposed where the particles hit it). The detector allowed the scientists to determine the distribution of the alpha particles after they interacted with the foil.
Easy

61. Explain the difference between mass number and atomic number.

The number of protons in the nucleus of an atom is characteristic of a particular element. This discovery was so important to our understanding of atoms that the number of protons in the nucleus of an atom is called the atomic number. The mass number of an atom is the sum of the numbers of protons and neutrons in the nucleus. Given the mass number for a nucleus (and knowing the atomic number of that particular atom), you can determine the number of neutrons by subtracting the atomic number from the mass number.
Moderate

62. Explain the organization of electrons in an atom.

Electrons are organized according to their energies into sets called shells. Generally, the higher the energy of a shell, the farther it is (on average) from the nucleus. Shells do not have specific, fixed distances from the nucleus, but an electron in a higher-energy shell will spend more time farther from the nucleus than does an electron in a lower-energy shell. Shells are further divided into subsets of electrons called subshells. The first shell has only one subshell, the second shell has two subshells, the third shell has three subshells, and so on. The subshells of each shell are labeled, in order, with the letters s, p, d, and f. Thus, the first shell has only an s subshell, the second shell has an s and a p subshell, the third shell has s, p, and d subshells, and so forth.
Moderate

63. Define core and valence electrons with an example.

Valence shell electrons (or, more simply, the valence electrons) are the electrons in the highest-numbered shell, or valence shell, while core electrons are the electrons in lower-numbered shells. We can see from the electron configuration of a carbon atom—1s22s22p2—that it has 4 valence electrons (2s22p2) and 2 core electrons (1s2).
Moderate

• Explain the classification of elements according to the periodic table.

Every element can be classified as a metal, a nonmetal, or a semimetal. A metal is a substance that is shiny, typically (but not always) silvery in color, and an excellent conductor of electricity and heat. Metals are also malleable and ductile. A nonmetal is typically dull and a poor conductor of electricity and heat. Solid nonmetals are also very brittle. Metals occupy the left three-fourths of the periodic table, while nonmetals (except for hydrogen) are clustered in the upper right-hand corner of the periodic table. The elements with properties intermediately between those of metals and nonmetals are called semimetals (or metalloids).
Moderate

65. What explains the similarities of elements in a periodic table?

Starting with the first period and going from left to right, the table reproduces the order of filling of the electron subshells in atoms. Furthermore, elements in the same column share the same valence shell electron configuration. Chemistry is largely the result of interactions between the valence electrons of different atoms. Thus, atoms that have the same valence shell electron configuration will have similar chemistry.
Moderate

 

Fill in the Blanks

66. The most abundant element on the earths crust is _____.

 oxygen; Easy

67. The chemical symbol for tungsten is _____.

W; Easy

68. The element represented by the symbol Cr is _____.

chromium; Easy

69. A(n) _____ is the smallest part of an element that maintains the identity of that element..

atom; Easy

70. _____ is a fundamental concept that states that all elements are composed of atoms.

Modern atomic theory; Easy

71. The mass number is the sum of protons and _____.

neutrons; Easy

72. 1s22s22p63s1 is the electronic configuration of _____.

sodium; Moderate

73. Rutherford called his description of the atom the _____.

planetary model; Easy

74. Atomic radius _____ down a row in the periodic table.

increases; Easy

75. Carbon has 2 core and _____ valence electrons.

4; Easy

 

 

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Elements atoms periodic table answers

 

 

Elements atoms periodic table answers

 

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