Trends in the Periodic Table

Question 1

What is atomic radius?

Answer 1

The distance from the nucleus of an atom to the outermost shell of electrons.

Question 2

True or False: Atomic radius increases down a group in the periodic table.

Answer 2

True

Question 3

What trend does atomic radius follow across a period from left to right?

Answer 3

Atomic radius decreases.

Question 4

Fill in the blank: Electronegativity is the ability of an atom to attract ______ in a chemical bond.

Answer 4

electrons

Question 5

Which element has the highest electronegativity?

Answer 5

Fluorine

Question 6

True or False: Electronegativity generally increases down a group.

Answer 6

False

Question 7

What is the trend of first ionisation energy as you move down a group?

Answer 7

First ionisation energy decreases.

Question 8

What happens to first ionisation energy as you move across a period from left to right?

Answer 8

First ionisation energy increases.

Question 9

Which factor primarily influences atomic radius?

Answer 9

The number of electron shells.

Question 10

Multiple Choice: Which of the following elements has the largest atomic radius? a) Lithium b) Sodium c) Potassium d) Rubidium

Answer 10

d) Rubidium

Question 11

Short Answer: What is the general trend of electronegativity across a period?

Answer 11

Electronegativity increases.

Question 12

Fill in the blank: The first ionisation energy is the energy required to remove the most loosely bound ______ from an atom.

Answer 12

electron

Question 13

True or False: Noble gases have high electronegativity.

Answer 13

False

Question 14

What is the trend of electronegativity down a group?

Answer 14

Electronegativity decreases.

Question 15

Which group of elements typically has the highest first ionisation energies?

Answer 15

Noble gases

Question 16

Multiple Choice: Which of the following has the highest first ionisation energy? a) Magnesium b) Calcium c) Beryllium d) Strontium

Answer 16

c) Beryllium

Question 17

Short Answer: Why does atomic radius decrease across a period?

Answer 17

Increased nuclear charge pulls electrons closer.

Question 18

What is the relationship between atomic radius and ionisation energy?

Answer 18

As atomic radius decreases, ionisation energy increases.

Question 19

True or False: Transition metals generally have lower electronegativity than alkali metals.

Answer 19

False

Question 20

Fill in the blank: The trend of atomic radius is primarily due to changes in ______.

Answer 20

effective nuclear charge

Question 21

Which element has the lowest electronegativity?

Answer 21

Cesium

Question 22

Multiple Choice: Which element would likely have the lowest first ionisation energy? a) Fluorine b) Neon c) Sodium d) Argon

Answer 22

c) Sodium

Question 23

Short Answer: What is the effect of increasing electron shielding on ionisation energy?

Answer 23

It decreases ionisation energy.

Question 24

What trend does ionisation energy follow as you move from top to bottom in a group?

Answer 24

Ionisation energy decreases.

Question 25

True or False: The atomic radius of nonmetals is generally larger than that of metals.

Answer 25

False

Question 26

Fill in the blank: The ability of an atom to attract electrons in a bond is known as ______.

Answer 26

electronegativity

Question 27

Which element has a larger atomic radius: Chlorine or Bromine?

Answer 27

Bromine

Question 28

What is an emission spectrum?

Answer 28

An emission spectrum is a spectrum of the electromagnetic radiation emitted by a source.

Question 29

What is an absorption spectrum?

Answer 29

An absorption spectrum is a spectrum of absorbed light, showing the wavelengths of light absorbed by a substance.

Question 30

True or False: An emission spectrum appears as a continuous range of colors.

Answer 30

False

Question 31

Fill in the blank: The emission spectrum consists of _____ lines at specific wavelengths.

Answer 31

spectral

Question 32

What causes the lines in an emission spectrum?

Answer 32

The lines are caused by electrons transitioning between energy levels in an atom.

Question 33

Multiple choice: Which of the following is NOT a type of spectrum? A) Continuous B) Emission C) Absorption D) Reflection

Answer 33

D) Reflection

Question 34

What is the relationship between absorption and emission spectra?

Answer 34

Absorption and emission spectra are complementary; the wavelengths absorbed in an absorption spectrum correspond to the wavelengths emitted in an emission spectrum.

Question 35

True or False: The absorption spectrum can be used to identify the elements in a star.

Answer 35

True

Question 36

What is the significance of the Balmer series?

Answer 36

The Balmer series is a specific set of spectral lines corresponding to electron transitions in hydrogen.

Question 37

Fill in the blank: The _____ effect describes the shift in the wavelength of light from an object moving away from an observer.

Answer 37

Doppler

Question 38

Multiple choice: The emission spectrum of which element consists of distinct lines? A) Hydrogen B) Air C) Water D) Salt

Answer 38

A) Hydrogen

Question 39

Short answer: What is a continuous spectrum?

Answer 39

A continuous spectrum is a spectrum that shows all wavelengths of visible light without any gaps.

Question 40

True or False: Absorption lines appear as dark lines on a continuous spectrum.

Answer 40

True

Question 41

What role does temperature play in the emission spectrum of a substance?

Answer 41

Temperature affects the energy levels and transitions of electrons, altering the emission spectrum.

Question 42

Fill in the blank: The study of emission and absorption spectra is known as _____ spectroscopy.

Answer 42

spectroscopy

Question 43

What is the main tool used to observe emission and absorption spectra?

Answer 43

A spectroscope or spectrometer.

Question 44

Multiple choice: Which type of spectrum is produced when light passes through a cold gas? A) Emission B) Absorption C) Continuous D) None of the above

Answer 44

B) Absorption

Question 45

Short answer: Why do different elements produce different emission spectra?

Answer 45

Different elements have unique electron configurations, leading to different energy level transitions.

Question 46

True or False: The emission spectrum of an element can change under different conditions.

Answer 46

True

Question 47

Fill in the blank: The visible spectrum ranges from approximately _____ nm to _____ nm.

Answer 47

400, 700

Question 48

What is the photoelectric effect?

Answer 48

The photoelectric effect is the emission of electrons from a material when it absorbs light.

Question 49

Multiple choice: Which of the following best describes a line spectrum? A) A spectrum with a smooth gradient B) A spectrum with discrete lines C) A spectrum with no visible light D) A spectrum with all colors

Answer 49

B) A spectrum with discrete lines

Question 50

What is the formula used to calculate the wavelength of light emitted during an electron transition?

Answer 50

The Rydberg formula.

Question 51

Fill in the blank: The _____ of an atom determines how it interacts with light.

Answer 51

electronic structure

Question 52

True or False: Emission spectra can be used to determine the composition of distant stars.

Answer 52

True