C1(Atomic Structure) Flashcards

1
Q

What is an atom?

A

An atom is the basic unit of matter, made up of protons, neutrons, and electrons.

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2
Q

What are the subatomic particles of an atom?

A

The subatomic particles are:

Protons (positive charge, located in the nucleus)
Neutrons (no charge, located in the nucleus)
Electrons (negative charge, orbit the nucleus)

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3
Q

What is the relative mass and charge of a proton?

A

Relative mass: 1
Charge: +1

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4
Q

What is the relative mass and charge of a neutron?

A

Relative mass: 1
Charge: 0

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5
Q

What is the relative mass and charge of an electron?

A

Relative mass: 1/1836(practically nothing )
Charge: -1

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6
Q

What is the atomic number?

A

The atomic number is the number of protons in an atom’s nucleus. It determines the element.

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7
Q
A
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8
Q

What is the mass number?

A

The mass number is the total number of protons and neutrons in an atom’s nucleus.

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9
Q

How do you calculate the number of neutrons in an atom?

A

Number of neutrons = Mass number - Atomic number

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10
Q

What is an isotope?

A

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.

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11
Q

What is an ion?

A

An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a charged particle.

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12
Q

What is a positive ion (cation)?

A

An atom that has lost electrons, resulting in a positive charge.

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13
Q

What is a negative ion (anion)?

A

An atom that has gained electrons, resulting in a negative charge.

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14
Q

How is an atom arranged ?

A

The protons and neutrons are in the nucleus in the centre with electrons orbiting the nucleus at fixed rates.

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15
Q

What is the electronic configuration of an atom?

A

The electronic configuration shows the arrangement of electrons in an atom’s energy levels (shells).

Example: Oxygen (atomic number 8) has the electronic configuration 2, 6.

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16
Q

What is the maximum number of electrons that can fit in the first three electron shells?

A

1st shell: 2 electrons
2nd shell: 8 electrons
3rd shell: 8 electrons

17
Q

What is the periodic table?

A

The periodic table is an arrangement of elements in order of increasing atomic number, where elements with similar properties are grouped in columns (groups).

18
Q

What are the groups in the periodic table?

A

Groups are vertical columns in the periodic table. Elements in the same group have similar chemical properties because they have the same number of electrons in their outer shell.

19
Q

What are the periods in the periodic table?

A

Periods are horizontal rows in the periodic table. As you move across a period, the atomic number increases, and elements change from metals to non-metals.

20
Q

What is the charge of an atom in its neutral state?

A

An atom in its neutral state has no charge because the number of protons equals the number of electrons.

21
Q

What is the relationship between protons and electrons in a neutral atom?

A

In a neutral atom, the number of protons equals the number of electrons.

22
Q

What is the use of the atomic number in the periodic table?

A

The atomic number determines the element’s identity and its position in the periodic table. It indicates the number of protons in an atom’s nucleus.

23
Q

What is a chemical symbol?

A

A chemical symbol is a one- or two-letter notation used to represent an element.

For example, O for oxygen, Na for sodium.

24
Q

How is the structure of the atom related to its position in the periodic table?

A

The number of electrons and the arrangement of electrons in an atom’s energy shells determine its chemical properties and position in the periodic table.

25
Q

What is a mass spectrometer used for?

A

A mass spectrometer is used to determine the relative abundance and mass of isotopes of an element.

26
Q

What is the relative atomic mass?

A

The relative atomic mass is the weighted average mass of the isotopes of an element, relative to the mass of a carbon-12 atom.

27
Q

What is the difference between relative atomic mass and mass number?

A

Relative atomic mass: The average mass of an element’s atoms, taking into account isotopes.
Mass number: The total number of protons and neutrons in a specific isotope.

28
Q

What is an ionization energy?

A

Ionization energy is the energy required to remove one mole of electrons from one mole of atoms in their gaseous state.

29
Q

What trends are observed in the periodic table in terms of atomic size, ionization energy, and electronegativity?

A

Atomic size: Increases down a group and decreases across a period.
Ionization energy: Decreases down a group and increases across a period.
Electronegativity: Decreases down a group and increases across a period.

30
Q

What are the noble gases, and why are they unreactive?

A

The noble gases (Group 18) are chemically inert because their outer electron shells are full, making them stable and unlikely to form bonds.

31
Q

What is the Bohr model of the atom?

A

The Bohr model suggests that electrons orbit the nucleus in fixed paths or energy levels (shells).

32
Q

What is the Rutherford model of the atom?

A

The Rutherford model proposed that an atom has a small, dense nucleus containing protons, with electrons orbiting outside the nucleus.

33
Q

What was the discovery of the electron?

A

The electron was discovered by J.J. Thomson in 1897 through experiments with cathode rays.

34
Q

How would you balance this equation : ‘Mg +02 —> Mg0 ‘?

A

2Mg + 02 —-> 2Mg0

35
Q

How to calculate Relative Atomic Mass(Ar)?